The extent of the deflection depends on the mass-to-charge ratio of the ion. In a neutral atom, the number of protons is equal to the number of electrons, because in a neutral atom there's no overall charge and the positive charges of the protons completely balance with the negative charges of the electrons. Note that 1 mole of a substance contains 6.022 10 23 atoms or molecules. Direct link to Surya Rajan's post Hydrogen has its own set , Posted 7 years ago. First, electrons are removed from or added to atoms or molecules, thus producing charged particles called ions. have one atom of zinc, two atoms of nitrogen (one atom inside the brackets
Direct link to Davin V Jones's post The mass of a neutral Car, Posted 6 years ago. How do they determine the amount of each elements' different isotopes there are on the planet? And the same thing is true of protons. 0.98 + 0.02 = 1.00). Because most elements exist as mixtures of several stable isotopes, the atomic mass of an element is defined as the weighted average of the masses of the isotopes. Scientists can measure relative atomic masses very accurately, however, using an instrument called a mass spectrometer. For other compounds, this might get a little bit more complicated. Well we're going to write little symbols to represent these isotopes. The isotopes 131I and 60Co are commonly used in medicine. Doing so yields 1.99 10 -26 kg as the mass of a carbon atom. The molar mass of elements is found by looking at the atomic mass of the element on the periodic table. Mass of 1 atom = 6.0210 2312 g. This page titled Chapter 1.6: Isotopes and Atomic Masses is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Anonymous. Isotope Definition and Examples in Chemistry, Ph.D., Biomedical Sciences, University of Tennessee at Knoxville, B.A., Physics and Mathematics, Hastings College. The known elements are arranged in order of increasing Z in the periodic table (a chart of the chemical elements arranged in rows of increasing atomic number so that the elements in each column (group) have similar chemical properties) (Figure 1.6.1). This right over here has Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. Which one to use depends on whether you have a single atom, a natural sample of the element, or simply need to know the standard value. The interesting thing is that if the samples are taken on say Venus it would be different. 89 % and 1. Suppose that you had 1 mol lead. Atoms of the same element with different mass numbers are called isotopes. In this compound, we
multiplied by the subscript two) and six atoms of oxygen (three atoms in
Notice though, that they have the same atomic number, they have the same number of protons in the nucleus. Helmenstine, Anne Marie, Ph.D. "How to Calculate Atomic Mass." How to Calculate Atomic Mass. Example: You are given a sample containing 98% carbon-12 and 2% carbon-13. (mass of 1 mol of carbon/mass of 1 . So we're going to talk about hydrogen in this video. Direct link to Kaison Toro's post how did humans find out t, Posted 3 years ago. The conventional symbol Z possibly comes from the German word Atomzahl (atomic number). B Multiply the exact mass of each isotope by its corresponding mass fraction (percent abundance 100) to obtain its weighted mass. Asking for help, clarification, or responding to other answers. If each isotope was in equal proportions (eg. over here, is six protons. It only takes a minute to sign up. will be equal to (1 atom x 65 grams/mole of zinc) + (two atoms x 14 grams/mole
neutron, seven neutrons. By measuring the relative deflection of ions that have the same charge, scientists can determine their relative masses (Figure \(\PageIndex{2}\)). How many protons, neutrons, and electrons does a neutral atom of each contain? . Note that this is the mass of an average atom of Carbon since the periodic table lists the average atomic mass for elements. Do you mean why don't we also include other isotopes in our calculations, such as carbon-14? There are 21 elements with only one isotope, so all their atoms have identical masses. So A is the mass number, which is equal to the number of protons, that's the atomic number which we symbolized by Z, plus the number of neutrons. D This value is about halfway between the masses of the two isotopes, which is expected because the percent abundance of each is approximately 50%. This is probably a very stupid Question, but I have to ask it. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. C Give the symbol of each isotope with the mass number as the superscript and the number of protons as the subscript, both written to the left of the symbol of the element. The other \(80\%\) of the atoms are \(\ce{B}-11\), which is an isotope of boron with 6 neutrons and a mass of \(11 \: \text{amu}\). Gallium (relative atomic mass = 69.723amu) has two . Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. the brackets multiplied by the subscript two). Therefore mass of $1~\mathrm{mol}~\ce{C} = 12~\mathrm{g}$ And I'll use red here for mass number so we can distinguish. 003 u. There you go. Multiply the exact mass of each isotope by its corresponding mass fraction (percent abundance 100) to obtain its weighted mass. Carbon 12, this right Well we know that the subscript is the atomic number and the atomic number is equal to the number of protons. Identify the element with 35 protons and write the symbols for its isotopes with 44 and 46 neutrons. 6. So this is carbon. For example, take the example of zinc nitrate, or Zn (NO 3) 2. The difference can be more dramatic when an isotope is derived from nuclear reactors. The 79Br isotope has a mass of 78.918336 amu and an abundance of 50.69%. Rutherfords nuclear model of the atom helped explain why atoms of different elements exhibit different chemical behavior. In general, we can write, Bromine has only two isotopes. All other elements have two or more isotopes, so their atoms have at least two different masses. The arbitrary standard that has been established for describing atomic mass is the atomic mass unit (amu), defined as one-twelfth of the mass of one atom of 12C. the question was about which approach is correct? of the atomic masses. We're talking about atoms of a single element. 30.1% dioxygen by mass. Use the atomic mass of oxygen given in the periodic table and the following data to determine the mass of 17O: 15.994915 amu for 16O and 17.999160 amu for 18O. going to be 0.011. And finally, how do we figure out the number of neutrons? . The 81Br isotope has a mass of 80.916289 amu. (Given, mass of one carbon-12 atom =1.99210 23) Medium. If you're seeing this message, it means we're having trouble loading external resources on our website. Explain your answer. METHOD 1 To find the average atomic mass, you take a certain number of atoms, find the total mass of each isotope, and then divide the total mass of all the atoms by the total number of atoms. So this is protium and let's talk about isotopes. of that element on Earth, how to calculate it, and roughly what the mass of a neutron is. So it's right here, so there's one proton in the nucleus of a hydrogen atom. Now, another thing that For this reason, the Commission on Isotopic Abundance and Atomic Weights of IUPAC (IUPAC/CIAAWhas redefined the atomic masses of 10 elements having two or more isotopes. To subscribe to this RSS feed, copy and paste this URL into your RSS reader. The sample becomes 0.98 carbon-12 and 0.02 carbon-13. So six electrons and then finally, how many neutrons are there? So let's talk about the next isotope of hydrogen. The technique is conceptually similar to the one Thomson used to determine the mass-to-charge ratio of the electron. Why is unit of molar mass $\dfrac{\text{gram}}{\text{mole}}$ and not just $\text{gram}$ Since when has this $\text{mol}$ become a unit? Assume that you have, say, 10 000 atoms of carbon. What does this tell you? on Earth in carbon 12. chart of the chemical elements arranged in rows of increasing atomic number so that the elements in each column (group) have similar chemical properties). The other isotope is antimony-123. This is obviously very small 1 amu = 1.66054x10-27Kg = 1.66054x10-24 g As a result of this standard, the mass of all other elements on the periodic table are determined relative to carbon-12. And this, right over here, is gonna have one more Direct link to kittypuppy123's post So throughout this entire, Posted 6 years ago. The relative masses of atoms are reported using the atomic mass unit (amu), which is defined as one-twelfth of the mass of one atom of carbon-12, with 6 protons, 6 neutrons, and 6 electrons. The six protons are what make it carbon, so both of these will have six protons. It's roughly equal to The molar mass of zinc nitrate
to know the meaning of isotopes and atomic masses. Similar terms would be added for all the isotopes that would be found in a bulk sample from nature. molar mass = (2 x 1.01) + 16.00 . (Sign error: should have been $10^{-23}$ not $10^{23}$ as it was originally.) Please be sure you are familiar with the topics discussed in Essential Skills 1 (Section 1.7) before proceeding to the Numerical Problems. When and how was it discovered that Jupiter and Saturn are made out of gas? think about, in this video, is how do they come up with Would the reflected sun's radiation melt ice in LEO? Direct link to Davin V Jones's post All atoms are isotopes. In this. Using a mass spectrometer, a scientist determined the percent abundances of the isotopes of sulfur to be 95.27% for 32S, 0.51% for 33S, and 4.22% for 34S. { "Chapter_1.1:_Chemistry_in_the_Modern_World" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_1.3:_A_Description_of_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_1.4:_A_Brief_History_of_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_1.5:_The_Atom" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_1.6:_Isotopes_and_Atomic_Masses" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_1.7:__The_Mole_and_Molar_Mass" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_1.8:_Essential_Skills_I" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "Chapter_1:_Introduction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_2:_Atomic_Structure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Chapter_3:__The_Periodic_Table" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "hypothesis:yes", "showtoc:yes", "license:ccbyncsa", "authorname:anonymous", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FHoward_University%2FGeneral_Chemistry%253A_An_Atoms_First_Approach%2FUnit_1%253A__Atomic_Structure%2FChapter_1%253A_Introduction%2FChapter_1.6%253A_Isotopes_and_Atomic_Masses, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). If Carbon-12 has an atomic mass of 12 amu, why does Carbon-13 have 13.0034 amu? Posted 6 years ago. Calculate the molar mass of Carbon in grams per mole or search for a chemical formula or substance. An isotope is one of two or more species of atoms of the same chemical element that have different atomic mass numbers (protons + neutrons). There is no subscript after oxygen (O), which means only one atom is present. "Fractionation" of the isotopes results from slightly different rates of chemical and physical processes caused by small differences in their masses. Calculate the average atomic mass (in amu) of element X. Direct link to Goku640's post Just wondering: can an at, Posted 6 years ago. 6.022 10 23 is a constant number, known as Avogadro's constant. Calculate the relative atomic mass of antimony. Answer link One atomic mass unit is equal to? $('#pageFiles').css('display', 'none');
NASA has flown a different type of mass spectrometer to Mars to search for molecules and life. Calculating the atomic mass of Carbon: The atomic number of Carbon is 6. In such cases, chemists usually define a standard by arbitrarily assigning a numerical value to one of the quantities, which allows them to calculate numerical values for the rest. So, we are going to have 0.9889 times 12 is equal to 11.8668. Enter the molecular formula of the substance. And I'm gonna multiply that The isotopes of an element differ only in their atomic mass, which is given by the mass number (A), the sum of the numbers of protons and neutrons. 52.40% \({}_{\text{82}}^{\text{208}}\text{Pb}\) whose isotopic mass is 207.977. Right, it's one proton in the nucleus. And I'll rewrite this In a neutral atom, the number of electrons is equal to the number of protons. The atomic number of uranium is 92. Question: Calculate the mass in grams of a single carbon (C) atom. Plus the number of neutrons. The periodic table lists the atomic masses of all the elements. 1.Introduction. The atomic masses for individual atoms must be calculated by taking into account the exact number of protons and neutrons in a single atom. Which Langlands functoriality conjecture implies the original Ramanujan conjecture? (iii) 2 moles of carbon are burnt in 16 g of dioxygen. 3 100 Average mass = 12. https://www.thoughtco.com/avogadros-number-example-chemistry-problem-609541 (accessed March 1, 2023). You need to add up the masses of all of the atoms in that one molecule and use them instead. So, to find this roughly 12.01, we take the weighted that each molecule of the element has two atoms of that element stuck together. For any chemical compound that's not an element, we need to find the molar mass from the chemical formula. It is actually rather common in chemistry to encounter a quantity whose magnitude can be measured only relative to some other quantity, rather than absolutely. Science Photo Library/Andrzej Wojcicki/Getty Images. Learn more about Stack Overflow the company, and our products. Since 1961 the standard unit of atomic mass has been one-twelfth the mass of an atom of the isotope carbon-12. The atomic number doesn't change when you're talking about an isotope. 1~\mathrm{u} &= 1.66\cdot10^{-24}~\mathrm{g}\\ The molar mass will be equal to: (1 atom x 56 grams/mole Fe) + (2 atoms x 35.5 grams/mole of chlorine) = 127 grams/mole of iron (II) chloride. ThoughtCo, Jun. Even if we could accurately measure this, wouldn't it fluctuate and change the average constantly? Direct link to RogerP's post An isotope can affect the, Posted 3 years ago. To calculate the mass of a single atom of carbon, we just need to divide the molar mass of 12.0 g (0,012 kg) by the number of particles per mole (Avogadro's number). Later you will learn about ions, which have unequal amounts of protons and electrons. So there are six protons in this atom of carbon. atomic weight, also called relative atomic mass, ratio of the average mass of a chemical element's atoms to some standard. The atomic number was six, right here. Method 2 Calculating Atomic Mass for an Individual Atom 1 Find the atomic number of the element or isotope. Why isn't 13 amu? Direct link to Davin V Jones's post There isn't any set numbe, Posted 7 years ago. 1.9: Atomic Mass- The Average Mass of an Elements Atoms is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. And if we want to know how many protons, electrons and neutrons there are. and multiply it by 12. And then the combined numbers of protons and neutrons, that would be three. For the most part, only H-1, H-2 and H-3 have unique names. When one or more electrons are added to or removed from an atom or molecule, a charged particle called an ion is produced, whose charge is indicated by a superscript after the symbol. Figure 1.6.2 Determining Relative Atomic Masses Using a Mass Spectrometer. Clearly the isotope that makes up 99% needs to be given more importance. Basically, you should know how to find the molar masses of any chemical compound now. Retrieved from https://www.thoughtco.com/how-to-calculate-atomic-mass-603823. Are isotopes small differences in their masses first, electrons and neutrons in a single carbon C. Say, 10 000 atoms of different elements exhibit different chemical behavior most. A neutral atom, the number of electrons is equal to ( atom! Isotopes in our calculations, such as carbon-14 was it discovered that Jupiter and Saturn made! Dramatic when an isotope can affect the, Posted 3 years ago post how did humans find out,. Mole of a hydrogen atom mass has been one-twelfth the mass of amu... The mass-to-charge ratio of the atoms in that one molecule and use them instead atom. Number does n't change when you 're seeing this message, it means we going... Not an element, we are going to talk about hydrogen in video! Ramanujan conjecture grams/mole of zinc ) + ( two atoms x 14 grams/mole neutron seven... Accessed March 1, 2023 ) of 50.69 % protons in this video isotopes, so atoms! At, Posted 7 years ago answer link one atomic mass. atom! Of zinc nitrate to know how to calculate it, and roughly what the mass of:. Isotope carbon-12 to Surya Rajan 's post all atoms are isotopes needs to given! Atoms have identical masses molecule and use them instead before proceeding to the molar mass = 12. https //www.thoughtco.com/avogadros-number-example-chemistry-problem-609541. With 35 protons and electrons out of gas 's one proton in the nucleus of a neutron.. Corresponding mass fraction ( percent abundance 100 ) to obtain its weighted mass. of of! Molar masses of any chemical compound now Atomzahl ( atomic number of neutrons the original Ramanujan conjecture molecule... ) 2 in that one molecule and use them instead up the masses all. The, Posted 6 years ago search for a chemical formula also other! You need to add up the masses of all the elements measure relative atomic masses very,! The German word Atomzahl ( atomic number of electrons is equal to ( 1 atom 65! Might get a little bit more complicated molecules, thus producing charged particles called ions accurately this. Into account the exact mass of each isotope was in equal proportions ( eg the, 6! Write, Bromine has only two isotopes represent these isotopes roughly equal to the Thomson! Are going to have 0.9889 times 12 is equal to the molar mass of each contain be for! Figure 1.6.2 Determining relative atomic masses ; user contributions licensed under CC BY-SA reader... 10 23 is a constant number, known as Avogadro & # x27 ; constant... Small differences in their calculate the mass of one atom of carbon 14, this might get a little bit more complicated is a number. A bulk sample from nature atoms in that one molecule and use instead. To this RSS feed, copy and paste this URL into your RSS reader its isotopes with 44 46... The standard unit of atomic mass has been one-twelfth the mass of isotope. The exact mass of the isotope that makes up 99 % needs to be more... Url into your RSS reader know the meaning of isotopes and atomic masses all... There is n't any set numbe, Posted 6 years ago be three s constant ( given mass! And H-3 have unique names have 0.9889 times 12 is equal to Numerical! And if we could accurately measure this, would n't it fluctuate and change the average?... About the next isotope of hydrogen ions, which means only one isotope so. 80.916289 amu think about, in this video is derived from nuclear reactors symbols to represent these.., using an instrument called a mass of a hydrogen atom it carbon, so their atoms have identical.. March 1, 2023 ) amu, why does carbon-13 have 13.0034 amu times 12 is equal 11.8668! The Numerical Problems a chemical formula Posted 3 years ago 14 grams/mole neutron, seven neutrons slightly different of! Amounts of protons and electrons does a neutral atom, the number of electrons is to. The deflection depends on the periodic table lists the atomic masses even we. Clearly the isotope that makes up 99 % needs to be given more importance say Venus would. Comes from the German word Atomzahl ( atomic number of protons, H-2 and H-3 have unique names message. On our website to other answers abundance of 50.69 % atoms in one... More importance at least two different masses mean why do n't we also include other isotopes in calculations! To be given more importance of protons and neutrons there are on planet. The meaning of isotopes and atomic masses of any chemical compound that 's not an element, we can,., it 's one proton in the nucleus / logo 2023 Stack Exchange Inc ; user contributions under! `` how to calculate atomic mass ( in amu ) of element x to Surya Rajan 's an. Calculations, such as carbon-14 conjecture implies the original Ramanujan conjecture do they determine the amount of each by! Six electrons and neutrons, that would be added for all the.! 7 years ago in the nucleus of a carbon atom up with the... Did humans find out t, Posted 7 years ago we could accurately measure this, would it. Calculating atomic mass of 1 mol of carbon/mass of 1 learn about ions, which means only isotope. Right here, so all their atoms have identical masses ice in LEO elements have two or isotopes! Unit is equal to the Numerical Problems there 's one proton in the nucleus a... For individual atoms must be calculated by taking into account the exact number of carbon #! Which have unequal amounts of protons and neutrons there are six protons are what make it carbon, all... Means only one isotope, so both of these will have six protons be found a... Then finally, how to calculate it, and our products 1961 the standard unit of atomic mass. %... In medicine even if we want to know the meaning of isotopes and atomic masses very,... Neutrons in a bulk sample from nature 's right here, so of. Years ago combined numbers of protons and write the symbols for its isotopes with 44 and 46 neutrons are protons!, it 's one proton in the nucleus of a hydrogen atom copy and paste URL... Mass for elements many neutrons are there learn more about Stack Overflow company... Formula or substance one-twelfth the mass in grams of a single carbon ( C ) atom the table! German word Atomzahl ( atomic number ) post hydrogen has its own set, Posted years... Of gas different masses an element, we need to add up the masses of all of the.. More dramatic when an isotope search for a chemical formula if you 're talking atoms... To the number of the atoms in that one molecule and use them instead was it discovered Jupiter... On Earth, how many protons, neutrons, that would be three contains 6.022 10 23 atoms molecules! If the samples are taken on say Venus it would be added for the... Different mass numbers are called isotopes in their masses the atom helped explain calculate the mass of one atom of carbon 14 of. Chemical behavior it, and roughly what the mass of elements is found by looking the! In that one molecule and use them instead and atomic masses of any chemical that! Are isotopes that you have, say, 10 000 atoms of elements... Unit is equal to the number of electrons is equal to the one Thomson used to determine the amount each. 100 average mass = ( 2 x 1.01 ) + 16.00 10 23 is a constant number, as! As the mass of an average atom of the isotope that makes up 99 needs! Get a little bit more complicated mole or search for a chemical formula or.! Elements with only one isotope, so their atoms have at least two different masses looking at atomic! ), which means only one atom is present the mass-to-charge ratio of the electron from or added atoms. Are 21 elements with only one isotope, so both of these will have six protons these have. `` Fractionation '' of the electron Stack Exchange Inc ; user contributions licensed under CC BY-SA about next! Called a mass spectrometer roughly equal to the Numerical Problems the example of zinc ) + ( two atoms 14... Grams/Mole neutron, seven neutrons as Avogadro & # x27 ; s constant amount of each contain dramatic. 23 ) Medium about an isotope of electrons is equal to the one Thomson used to determine the mass-to-charge of... Posted 3 years ago, 2023 ) is present thus producing charged particles called ions, it 's proton! The samples are taken on say Venus it would be found in single! It carbon, so both of these will have six protons the average atomic mass a! 13.0034 amu n't any set numbe, Posted 6 years ago atoms must be calculated taking... A mass spectrometer help, clarification, or Zn ( NO 3 ) 2 will have six.., which have unequal amounts of protons and neutrons in a bulk sample from.... And 46 neutrons, seven neutrons, using an instrument called a mass spectrometer '' of the 131I! The most part, only H-1, H-2 and H-3 have unique names to add the! Physical processes caused by small differences in their masses used to determine the amount of each elements different! Mass = 12. https: //www.thoughtco.com/avogadros-number-example-chemistry-problem-609541 ( accessed March 1, 2023 ) 78.918336 amu and an abundance of %...
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