Chemistry - Chapter Eleven Practice Test

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Calculate the mass of 1.000 mole of CaCl(2).

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Calculate grams in 3.0000 moles of CO(2).

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Calculate number of moles in 32.0 g of CH(4).

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Determine mass in grams of 40.0 moles of Na(2)CO(3).

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Calculate the percent composition of KNO(3).

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Calculate percent composition for H(2)SO(4).

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An oxide of chromium is found to have the following percent composition: 68.4% Cr and and 31.6% O. What is the compound's empirical formula?

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A sample with a molar mass of 34.00 g/mol is found to consist of 0.44g H and 6.92g O. Find its molecular formula.

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The percent composition of a compound was found to be 63.5% silver, 8.2% nitrogen, and 28.3% oxygen. Determine the compound's empirical formula.

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If 4.04g of N combine with 11.46g O to produce a compound with a molar mass of 108.0 g/mol, what is the molecular formula of this compound?

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( Percent composition, Molar mass, Molecular formula, Empirical formula ) is the percent by mass of each element in a compound.

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( Percent Composition, Avogadro's number, Molecular Formula, Molar Mass ) is the number 6.02 * 10^23, which is the number of representative particles in a mole.

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( Molar mass, Molecular Formula, Avogadro's Number, Percent Composition ) is the mass in grams of one mole of any pure substance.

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( molar mass, mole, hydrate, empirical formula ): the SI base unit used to measure the amount of a substance. It is the number of representative particles, carbon atoms, in exactly 12 g of pure carbon-12.

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( A hydrate, Molar mass, A mole, Empirical formula ) is a compound that has a specific number of water molecules bound to its atoms.

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( Empirical formula, Molecular formula ) is a formula that specifies the actual number of atoms of each element in one molecule or formula unit of the substance.

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( Empirical formula, Molecular formula ) is a formula that shows the smallest whole number mole ratio of the elements of a compound and may or may not be the same as the ( empirical formula, molecular formula ).

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Calculate percent composition of C(2)H(5)OH.

This test covers the mole, particle and mole conversions, molar mass with elements, molar mass with compounds, empirical formula, molecular formula, percent composition, and vocabulary.

Chemistry - Chapter Eleven Practice Test

Calculate the mass of 1.000 mole of CaCl(2).

Calculate grams in 3.0000 moles of CO(2).

Calculate number of moles in 32.0 g of CH(4).

Determine mass in grams of 40.0 moles of Na(2)CO(3).

Calculate the percent composition of KNO(3).

Calculate percent composition for H(2)SO(4).

An oxide of chromium is found to have the following percent composition: 68.4% Cr and and 31.6% O. What is the compound's empirical formula?

A sample with a molar mass of 34.00 g/mol is found to consist of 0.44g H and 6.92g O. Find its molecular formula.

The percent composition of a compound was found to be 63.5% silver, 8.2% nitrogen, and 28.3% oxygen. Determine the compound's empirical formula.

If 4.04g of N combine with 11.46g O to produce a compound with a molar mass of 108.0 g/mol, what is the molecular formula of this compound?

Percent composition Molar mass Molecular formula Empirical formula( Percent composition, Molar mass, Molecular formula, Empirical formula ) is the percent by mass of each element in a compound.

Percent Composition Avogadro's number Molecular Formula Molar Mass( Percent Composition, Avogadro's number, Molecular Formula, Molar Mass ) is the number 6.02 * 10^23, which is the number of representative particles in a mole.

Molar mass Molecular Formula Avogadro's Number Percent Composition( Molar mass, Molecular Formula, Avogadro's Number, Percent Composition ) is the mass in grams of one mole of any pure substance.

molar mass mole hydrate empirical formula( molar mass, mole, hydrate, empirical formula ): the SI base unit used to measure the amount of a substance. It is the number of representative particles, carbon atoms, in exactly 12 g of pure carbon-12.

A hydrate Molar mass A mole Empirical formula( A hydrate, Molar mass, A mole, Empirical formula ) is a compound that has a specific number of water molecules bound to its atoms.

Empirical formula Molecular formula( Empirical formula, Molecular formula ) is a formula that specifies the actual number of atoms of each element in one molecule or formula unit of the substance.

Empirical formula Molecular formula( Empirical formula, Molecular formula ) is a formula that shows the smallest whole number mole ratio of the elements of a compound and may or may not be the same as the empirical formula molecular formula( empirical formula, molecular formula ).

Calculate percent composition of C(2)H(5)OH.

( Percent composition, Molar mass, Molecular formula, Empirical formula ) is the percent by mass of each element in a compound.

( Percent Composition, Avogadro's number, Molecular Formula, Molar Mass ) is the number 6.02 * 10^23, which is the number of representative particles in a mole.

( Molar mass, Molecular Formula, Avogadro's Number, Percent Composition ) is the mass in grams of one mole of any pure substance.

( molar mass, mole, hydrate, empirical formula ): the SI base unit used to measure the amount of a substance. It is the number of representative particles, carbon atoms, in exactly 12 g of pure carbon-12.

( A hydrate, Molar mass, A mole, Empirical formula ) is a compound that has a specific number of water molecules bound to its atoms.

( Empirical formula, Molecular formula ) is a formula that specifies the actual number of atoms of each element in one molecule or formula unit of the substance.

( Empirical formula, Molecular formula ) is a formula that shows the smallest whole number mole ratio of the elements of a compound and may or may not be the same as the ( empirical formula, molecular formula ).