Complete the table below for calculating the molar mass of the ionic compound copper(II) bromide. Ion Formula Molar Mass Number of Moles Mass of Ion in Compound Cation g/mol X mol 63.55 g Anion g/mol X mol Molar mass copper(II) bromide : g/mol %3D

Q: Complete the table below for calculating the molar mass of the ionic compound magnesium bromide .…

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Q: A particular protein sample is found to have 1 atom of iron in its chemical formula. If the mass…

A: Mass percent expresses the solute concentration in any mixture. The division of weight of dissolved…

Q: Calculate the mass % of 2.50 g Na3PO4 + 10.0 g H2O

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Q: A flask contains 0.470 mol of liquid bromine, Br2. Determine the number of bromine molecules present…

A: It is given that there is 0.470 mol of liquid bromine.

Q: Complete the table below for calculating the molar mass of the ionic compound nickel(II) chloride.…

A: Answer:Molar mass of an ionic compound is equal to the sum of all the ions present in the molecule.

Q: The molar mass of argon is 1 atom/6.022 x 1023 mol 18 mol/g 39.95 g/mol 18 g/mol 6.022 x 1023…

A: Molar mass Molar mass can be define as the mass of one mole of a substance. It is expressed in…

Q: Determine the number of moles in 6.80 × 10²³ formula units of MgCl₂

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Q: many molecules were used

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Q: A flask contains 0.390 mol of liquid bromine, Br2. Determine the number of bromine molecules present…

A: Given, Number of moles = 0.390

Q: Determine the number of moles in 1.19 × 10²³ formula units of MgCl₂.

A: It is known that one mole of a substance is equal to 6.022×1023 formula units of that substance…

Q: Calculate the number of grams in 2.72 x 10^21 formula units of sodium nitrite

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Q: Calculate the molar mass of a transition metal oxalate with the formula XC204.2 H2O. The molar mass…

A: Given, Formula : XC2O4.2H2O  Molar mass of X = 58.71 g/mol Molar mass of C = 12.01 g/mol Molar mass…

Q: Complete the following table. Mass of Sample Moles of Sample Molecules in Sample Total Atoms in…

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Q: Complete the following table. Mass of Sample Moles of Sample Molecules in Sample Total Atoms in…

A: The question is based on mole concept The formula used and solution is given in the picture

Q: Complete the table below for calculating the molar mass of the compound disulfur decafluoride.

A: We have given a compound disulfur decafluoride. We have to complete the given table for calculating…

Q: A chemist is given a sample of the CuSO4 hydrate and asked to determine the empirical formula of it.…

A: Given,  Mass of hydrated CuSO4 = 42.75 g Mass of Unhydrated salt = 27.38 g  Formula of hydrate = ?

Q: Calculate the mass percent of 0.485 g of H, which reacts with oxygen to form 2.32 g H2

A: Formula to be used to calculate mass percent of hydrogen  is given  below Mass  % of hydrogen = mass…

Q: 2. Calculate the number of molecules of water in a 500.0-mL glass of water. (Note: assume density of…

A: • As per bartleby guidelines, I need to solve only first question in case of multiple questions…

Q: What is the molar mass of phosphorus pentachloride (PC15)? O 190.30 g/mol O 208.22 g/mol O 172.75…

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Q: Complete the table below for calculating the molar mass of the compound boron tribromide.   Molar…

A: Given -> Boron tribromide (BBr3) The molar mass of a compound is often calculated by adding the…

Q: Calculate percent composition from a compound formula. Determine the percent composition of each…

A: Given compound: K2CO3 We have to determine the percent composition of each element in K2CO3.

Q: Calculate the mass (in g) of sample. 9.85x1019 CCl2F2 molecules

A: The mass (in g) of sample 9.85x1019 CCl2F2 molecules can be calculated as

Q: You are given a 10.0 grams sample of ethanol (CH3CH2OH).   Explain how you can use the molar mass of…

A: The Avogadro’s number of any species is defined by a mole. The Avogadro’s number, NA, is equal to…

Q: Calculate the mass percent composition of Cu2(OH)2CO3

A: The objective of the question is to calculate the mass percent composition of each element in the…

Q: Part D. A 28.50 g sample of a compound of carbon, sulfur, hydrogen, and combusted (burned). 35.25 g…

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Q: Which of the following has the smallest mass? O 15.0 mol of F2 0.250 kg of Brz 425. g of Cl2 O 1.75…

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Q: Determine the number of moles in 4.00 × 10²³ formula units of MgCl₂

A: The given compound MgCl2 is made up of one magnesium atom and two chlorine atoms. One mole of…

Q: A sample of naphthalene was analyzed in the laboratory and it was determined that the sample…

A: Number of moles (mol) = Given mass (g)Molar mass (g/mol)Given that:Number of moles= 0.457 molesMolar…

Q: Determine the number of moles in 6.94 × 10²³ formula units of CaCl₂

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Q: 7. x = 4 atoms 1 mole 6.02 x 1023 atoms 23g 1 mole

A: The conversion of quantity from one unit system to another unit system is known as unit conversion.…

Q: Calculate the amount of  anions (in moles) in 5.0 g of magnesium bromate.

A: Magnesium bromate is Mg(BrO3)2. The ions present in magnesium bromate are Mg2+ and BrO3-. So, BrO3-…

Q: Calculate the mass (in g) of sample. 1 glucose molecule (C6H12O6)

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Q: What is the molecular formula of the following compound?   Empirical formula: CH2 (ℳ = 112.24…

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Q: Complete the following table. Mass of Moles of Sample Molecules in Sample Total Atoms in Sample…

A: Answer shown in attachment provide in explanation box Explanation:

Q: Molar mass of ion   Number of ions   Mass of ion in one mole of cobalt(III) sulfide Cation Co3+…

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Q: Calculate the percent composition by mass of each element in NaCio3. % Na = 23 % Cl = 35 % O = 48

A: The percent composition by mass of each element in NaClO3 is to be determined.

Q: Determine the number of moles in 4.74 × 10²³ formula units of MgCl₂.

A: Given, 4.74 × 10²³ formula units of MgCl₂

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.