Select the number of moles of NaCl in 8.68 x 1025 sodium chloride formula units. O 144 mol NaCl O 8.68 x 1025 mol NaCl O 8.68 mol NaCi O 0.00694 mol NaCl

Q: Which sample has the greatest mass of atomic oxygen?   36.0 g of H2O   1.0 mol of NO2   1.20 ×…

A: Three samples  are given:36.0 g of H2O1.0 mol of NO21.20 × 1024 molecules of O2

Q: How many atoms of hydrogen are in 1.00 mole of ammonia, NH3? 3.01 10^23 H atoms 9.03*10^23 H atoms…

A:

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: Calculate the mass in grams of 1 glucose molecule ( C6H12O6)

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Q: Calculate mass percent of each element in perchoric acid, HCLO4 ?

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Q: Calculate the number of grams of Carbon, C in 0.31 mol CgHsO+

A: In this equation, we want to determine the mass of Carbon in give molecule.  How to calculate it, I…

Q: what is the mass in grams of 4.31 x 10-3 mole (NH4)2HPO4

A: Mass of a substance can be determined with the number of moles and molar mass of the substance.

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

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Q: How many grams are in 8.2x10^22 molecules of N2I6

A: First calculate number of moles of N2I6 by dividing given number of molecules of N2I6 with…

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: How many moles are in 5.94 x 10^20 H2O2 molecules?

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Q: Complete the table below for calculating the molar mass of the compound carbon tetrachloride. Molar…

A: The complete table for the molar mass of the compound carbon tetrachloride is given below, 1mole of…

Q: This question will walk you through the process of calculating the empirical formula of a 100.0 g…

A: Given: The number of moles of carbon, nitrogen, and hydrogen present in 100 g of sample is 2.38 mol,…

Q: In a combustion analysis experiment, an unknown hydrocarbon produced 154.47861 g of carbon dioxide…

A: Empirical formula represents the smallest whole number ratio of the atoms present in the organic…

Q: The density of ammonia, NH3, is 7.71 x 104 g/mL. Calculate the number of moles of ammonia in a 31.9…

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Q: Phosphorus pentachloride, PCIs, a white solid that has a pungent, unpleasant odor, is used as a…

A: mole is equal to weight of substance divide by it's molar mass

Q: The empirical formula of a compound is X5Y7Q by mass and the molecular formula weighs 162.1 g/mol.

A: Let us the consider the actual molecular formula as (X5Y7Q)n. Then,n x ( 12.01*5 + 16*7 + 14.01) =…

Q: The formula of acetic acid is CH3COOH (alternatively written as C₂H4O₂). What is the molar mass of…

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Q: Complete the table below for calculating the molar mass of the compound tetraphosphorus decaoxide. P…

A: Given compound is tetraphosphorus decaoxide. The molecular formula of tetraphosphorus decaoxide =…

Q: Determine the mass in grams of 1.6x10-3 mol glucose, C6H12O6

A: Since the molar mass of glucose = Sum of atomic masses of all the atoms present in it  Since each…

Q: compound has the mass percent data given below . Determine its empirical formula. 32.43 % carbon by…

A: Empirical formula of a chemical compound is the simplest positive integer ratio of atoms present in…

Q: Calculate the number of moles in 3.34x10 34 molecules of Cu (OH)2

A: Mole is used to determine the amount of substance. One mole of a substance contains 6.022×1023…

Q: How many moles are in 3.56 x 10 ^25 molecules of carbon dioxide, CO2

A: Given: Molecules present are 3.56 × 1025

Q: Calculate the % composition by mass of each element in phosphorus oxychloride POCl3. Keep at least…

A: Mass composition explanation the amount  of each elements present in whole sample.

Q: Wine is approximately 12% ethanol (CH3CH2OH) by volume. Ethanol has a molar mass of 46.06 g/mol and…

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Q: An unknown compound contains only carbon, hydrogen, and oxygen. Combustion of a 16.45 mg sample…

A: mass of sample = 16.45 mg = 0.01645 g mass of CO2 = 38.93 mg = 0.03893 g mass of H2O= 15.93 mg =…

Q: What is the mass, in grams, of 6.5 x 10-3 moles of ammonium phosphate? 1.35 g 0.97 g 0.85 g 0.73 g

A: Concept:  Moles and molar mass can be used to predict the mass of the sample. Moles is unit to have…

Q: Determine the molecular and empirical formulas of a compound containing 141.34 g C, 25.893 g H, and…

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Q: Determine the empirical formula of the compound according to its elemental analysis:  38.13% C by…

A: Determination of empirical formula The percentage composition of elements present in given compound…

Q: How many molecules are in 2.49x10^3 g of CuSO4?

A: Given mass of CuSO4 = 2.49x103 g According to Avogadro's Number  1 mole=6.02×1023 molecules  molar…

Q: calculate the number of molecules in 0.256 g of NH4Cl. (molar mass of NH4Cl = 53.492 g/mol; 1 mole =…

A: Q. Given Ammonium Chloride (NH4Cl) compoundm = 0.256 g ( given mass of Ammonium Chloride)M = 53.492…

Q: Complete the table below for calculating the molar mass of the compound phosphorus triiodide. Molar…

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Q: How many moles are in a sample of ethanol, CH 3CH 2OH that has a volume of 100.0 mL? The molar mass…

A: Mass of ethanol can be determined as follows:

Q: What is the molar mass of sodium phosphate, Na 3PO 4?     119.0 g     354.0 g     226.0 g…

A: Mole concept: The number of molecules or atoms present in the one mole of the substance is equal to…

Q: Determine the quantity of moles in 4.21 x 10^23 formula units of CaCl2

A: Given,number of formula units of CaCl2 = 4.21 x 1023

Q: Determine the mass in grams of 1.6 × 10⁻³ mol glucose , C₆H₁₂O₆

A: Molecular formula of glucose is . That means 1 mole of glucose weighs -------- 180g.

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.