1. A sample of hydrogen gas (H2) has a volume of 8.56 L at a temperature of 0 ̊C and a pressure of 1.5 atm. Calculate the moles of H2 molecules present in this gas sample. 2. Suppose we have a sample of ammonia gas (NH3) with a volume of 7.0 mL at a pressure of 1.68 atm. The gas is compressed to a volume of 2.7 mL at a constant temperature. Use the ideal gas law to calculate the final pressure. 3. A sample of methane gas that has a volume of 3.8 L at 5 ̊C is heated to 86 ̊C at constant pressure. Calculate its new volume. Chemistry 1_Q3 Page 6 4. A sample of diborane gas (B2H6), a substance that bursts into flame when exposed to air, has a pressure of 345 torr at a temperature of -15 ̊C and a volume of 3.48 L. If conditions are changed so that the temperature is 36 ̊C and the pressure is 468 torr, what will be the volume of the sample? Use the formula for combined gas laws: P1V1 T1 = P2V2 T2 5. A sample containing 0.35 mol argon gas at a temperature of 13 ̊C and a pressure of 568 torr is heated to 56 ̊C and a pressure of 897 torr. Calculate the change in volume that occurs. Tip: Use the ideal gas law equation twice, using different temperature in each calculation. 6. What is the density of nitrogen gas (N2) at 248.0 Torr and 18 ̊C? Tip: Density is mass/volume. ρ = PM RT = (pressure)(molar mass) (gas constant)(temperature) 7. Find the volume, in mL, when 7.00 g of O2 and 1.50 g of Cl2 are mixed in a container with a pressure of 482 atm and at a temperature of 22 ̊C. Tip: Add the moles of O2 and Cl2 to get the total n.
1. A sample of hydrogen gas (H2) has a volume of 8.56 L at a temperature of 0 ̊C and a
pressure of 1.5 atm. Calculate the moles of H2 molecules present in this gas sample.
2. Suppose we have a sample of ammonia gas (NH3) with a volume of 7.0 mL at a pressure
of 1.68 atm. The gas is compressed to a volume of 2.7 mL at a constant temperature. Use
the
3. A sample of methane gas that has a volume of 3.8 L at 5 ̊C is heated to 86 ̊C at
constant pressure. Calculate its new volume.
Chemistry 1_Q3 Page 6
4. A sample of diborane gas (B2H6), a substance that bursts into flame when exposed to air,
has a pressure of 345 torr at a temperature of -15 ̊C and a volume of 3.48 L. If conditions
are changed so that the temperature is 36 ̊C and the pressure is 468 torr, what will be the
volume of the sample? Use the formula for combined
T1
=
P2V2
T2
5. A sample containing 0.35 mol argon gas at a temperature of 13 ̊C and a pressure of
568 torr is heated to 56 ̊C and a pressure of 897 torr. Calculate the change in volume that
occurs. Tip: Use the ideal gas law equation twice, using different temperature in each
calculation.
6. What is the density of nitrogen gas (N2) at 248.0 Torr and 18 ̊C? Tip: Density is
mass/volume. ρ =
PM
RT
=
(pressure)(molar mass)
(gas constant)(temperature)
7. Find the volume, in mL, when 7.00 g of O2 and 1.50 g of Cl2 are mixed in a container with
a pressure of 482 atm and at a temperature of 22 ̊C. Tip: Add the moles of O2 and Cl2 to
get the total n.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
