ch. 6 (1-24)

which of the following defines standard temperature

0 degrees celsius

6.00 g of water contains how many moles of water

0.333 mol

which represents the greatest mass

1.0 mol Zn

calculate the number of moles of water molecules of 25.0 g of water

1.39 mol

convert 48 g to mol O2

1.5 mol

the mass of 0.80 mol of H2 is

1.6 g

what is the mass of 2.00 moles of Ca(OH)^2

148.2 g

6.00 g of water contains how many molecules of water

2.01 x 10^23

how many moles of Ca atoms are in 801 g Ca

20.0 mol

one mole of CO2 at STP will occupy

22.4 L

what volume will 28.0 g of N2 occupy at STP

22.4 L

the mass percent of oxygen in CaO is

28.5%

a 20.0 g sample of Ca contains how many calcium atoms

3.0 x 10^23

a 1.0 mole sample of H2O2 weighs

34 g

what is the percent (by mass) of carbon in glucose C6H12O6

40.0%

One mole of something consists of _____ units of that substance.

6.02 x 10^23

how many atoms are in a sample of an element whose mass in grams is numerically equal to the atomic mass

6.02 x 10^23

the molar mass of calcium hydroxide is

74.1 g

a hydrocarbon has the formula C2H4. what is the percent by mass of carbon in the compound?

85.6%

how many liters of O2 are there in 4.0 mol of O2

89.6

the mass in grams of 6.02 x 10^23 particles of a substance is called its

molar mass

the number of atoms of an element equal to the number of atoms in exactly 12.0 grams of carbon-12 is called

mole

the atomic mass of individual atoms is generally expressed in which unit

amu

the scale for expressing atomic mass is based on the mass of

carbon-12