TRUE/FALSE QUESTIONS FOR CHAPTER 6

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The empirical formula for C₆H₆ is C₃H₃.

FALSE

One mole of CO₂ gas contains 1 mole of carbon atoms and 2 moles of oxygen atoms.

TRUE

An empirical formula gives the specific number of each type of atom in a molecule.

FALSE

One hundred nickels must have the same mass as one hundred pennies.

FALSE

One mole of argon has more atoms in it than one mole of neon.

FALSE

One mole of chlorine gas has a mass of 35.45 grams.

FALSE

One mole of water contains 6.022 × 10²³ hydrogen atoms.

FALSE

One mole of zinc contains 65.39 zinc atoms.

FALSE

The chemical formula CuBr₂ indicates that this compound is composed of 1 gram of copper and 2 grams of bromine.

FALSE

The chemical formula clearly indicates the relationship between the mass of each element in the formula.

FALSE

The correct formula for calculating mass percent of X in compound XY is: Mass of X in a sample of the compound/ Mass of Y in a sample of the compound= Mass % X

FALSE

The empirical formula mass must be 25.0 if the molecular formula mass is 250 and n = 5.

FALSE

The mass of 2.0 moles of H₂O is greater than the mass of 1.0 mole of CO₂.

FALSE

The mole has a value of 6.023 × 10²².

FALSE

The number 6.022 × 10²³ is six times larger than the number 6.022 ×10²².

FALSE

A molecule that has an empirical formula of HO and a molar mass of 34.02 gram must have a molecular formula of H₂O₂.

TRUE

An empirical formula gives the smallest whole number ratio of each type of atom in a molecule.

TRUE

Avogadro's Number is 6.022 × 10²³

TRUE

C₂H₃O₂ could be an empirical formula.

TRUE

C₂H₆O₃ could be an empirical formula.

TRUE

Mass is used as a method of counting atoms.

TRUE

One mole of I₂ has more atoms in it than one mole of Na.

TRUE

One mole of copper atoms is 6.022 × 10²³ copper atoms.

TRUE

One mole of lead(II) nitrate contains six moles of oxygen atoms.

TRUE

One mole of nitrogen gas contains (2) × (6.022 × 10²³) nitrogen atoms.

TRUE

One mole of water contains 16 grams of oxygen atoms.

TRUE

The numerical value of the mole is defined as being equal to the number of atoms in exactly 12 grams of pure carbon-12.

TRUE

There are 6 grams of carbon in 22 grams of carbon dioxide.

TRUE

Two moles of cobalt atoms have a mass of 117.87 grams.

TRUE

Six grams of carbon contains 3.008 × 10²³ atoms.

TRUE

The empirical formula mass is 18.0 and the molecular formula mass is 90, therefore n = 5.

TRUE

The lighter the atom, the less mass in one mole of that atom.

TRUE

The molar mass of a compound in grams per mole is numerically equal to the formula mass of the compound in atomic mass units.

TRUE

The molar mass of a compound serves as a conversion factor between grams and moles.

TRUE

The molecular formula is equal to the empirical formula multiplied by a whole number integer.

TRUE

Water is 11.2% hydrogen by mass.

TRUE

C₂H₆O₄ could be an empirical formula.

FALSE


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