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If the atmospheric pressure is 97.4 kPa, how much is it in mm Hg? In atm? In torr?
A gas has an initial volume of 39 mL at an unknown pressure. If the same sample
occupies 514 mL at 720 torr, what was the initial pressure?
Calculate the missing variable in each set.
V1 = 2.0 L, T1 = 15°C, V2 = ?, T2 = 34°C
V1 = ?, T1 = 149°C, V2 = 310 mL, T2 = 54°C
V1 = 150 L, T1 = 180 K, V2 = 57 L, T2 = ?
A bicycle tire is inflated to a pressure of 3.74 atm at 15°C. If the tire is heated to
35°C, what is the pressure in the tire? Assume the tire volume doesn’t change.
How many moles of an ideal gas are there if the volume of the gas is 158 L at
14°C and a pressure of 89 kPa?
Calculate the mass in gram of each of the following gases at STP: (a) 1.4 L of
SO2 (b) 3.5 105 L of CO2
For a gas sample whose total pressure is 740 torr, what are the partial pressures if
the moles of gas present are 1.3 mol of N2, 0.33 mol of O2, and 0.061 mol of Ar?
A sample of gas is made entirely of carbon dioxide and water, and there are 259
moles of CO2 and 513 moles of water. If the total pressure of the sample is 21
atm, what is the partial pressure of each gas?
An experiment is being carried out to test the removal of sulfur dioxide from
gases being released by a power plant. The initial sample, which contains only
carbon dioxide and sulfur dioxide, occupies a volume of 35 L at a temperature of
41°C and a pressure of 715 torr. After all of the SO2 has been removed, the
sample occupies a volume of 23.5 L at a temperature of 29°C and a pressure of
715 torr. Determine the partial pressures of both CO2 and SO2 in the initial
The first step in processing zinc metal from its ore, ZnS, is to react it with O2
according to the reaction
2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g)
If 620 kg of ZnS is to be reacted, what volume of oxygen at 0.977 atm and
34.0°C is needed (at a minimum) to carry out this reaction?
If boron hydride, B4H10, is treated with pure oxygen, it burns to give B2O3 and
2 B4H10(s) + 11 O2(g) → 4 B2O3(s) + 10 H2O(g)
If a 0.050-g sample of the boron hydride burns completely in O2, what will be the
pressure of the gaseous water in a 4.25-L flask at 30.0°C?
Consider the following reaction:
6 NiO(s) + 4 ClF3(g) → 6 NiF2(s) + 2 Cl2(g) + 3 O2(g)
What mass of NiO will react with a sample of ClF3 gas that has a pressure of 250
torr in a 2.5-L flask at 20°C?
You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature
(25°C). Calculate the pressure the gas would have using (a) the ideal gas law and
(b) the van der Waals equation. (For CO2, a = 3.59 atm L2/mol2 and
b = 0.0427 L/mol.)
Nitric acid can be prepared by bubbling dinitrogen pentoxide into water.
N2O5(g) + H2O( ) → 2 H+(aq) + 2 NO3–(aq)
(a) How many moles of H+ are obtained when 1.50 L of N2O5 at 25°C and 1.00
atm pressure is bubbled into water? (b) The solution obtained in (a) after reaction
is complete has a volume of 437 mL. What is the molarity of the nitric acid
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