The combined and ideal gas laws
Grade 10 Science Worksheet - Challenge Me
Circle the best answer, or write your answer on the line.
A 5 L balloon at 101.3 kPa and 20 °C rises to where it is 80 kPa and 5 °C. What is its new volume, to 0.01 L, Esme?
A 2 L sealed bag at 1 atm and 25 °C ends at 2.5 atm and 50 °C. What is its new volume, to 0.01 L, Jun?
A 3 L balloon at 100 kPa and 27 °C ends at 150 kPa and 127 °C. What is its new volume, to 0.01 L, Kira?
Pia says PV = nRT gives about 22.4 L for 1 mol of gas at 0 °C and 1 atm. Which reply fits, Milo?
- Disagree: each gas has its own molar volume at 0 °C
- Disagree: PV = nRT gives 8.314 L
- Agree: V = 1 × 0.08206 × 273.15 ÷ 1 = 22.41 L
Tala says doubling the moles of gas in a rigid box at the same temperature doubles the pressure. Which reply fits, Noah?
- Disagree: the pressure halves as n doubles
- Disagree: moles do not affect pressure
- Agree: P = nRT ÷ V, so P doubles with n
A 1.00 L sealed flask holds 1.80 g of CO₂ at 1.00 atm and 27 °C. What molar mass does PV = nRT give, Pia?
- About 4.0 g/mol, using 27 instead of 300.15
- About 44.3 g/mol, close to CO₂'s 44.01
- About 4492 g/mol, using 8.314
1.00 L of O₂ at 1.00 atm and 0 °C has a mass of 1.43 g. What molar mass does PV = nRT give, Ren?
- About 1.43 g/mol, the mass itself
- About 32.1 g/mol, close to O₂'s 32.00
- About 0.04 g/mol, from the moles alone
A 2.00 L balloon holds 2.33 g of N₂ at 1.00 atm and 20 °C. What molar mass does PV = nRT give, Tala?
- About 28.0 g/mol, close to N₂'s 28.02
- About 1.9 g/mol, using 20 instead of 293.15
- About 2839 g/mol, using 8.314
Two balloons have the same volume, pressure and temperature: one of O₂, one of CO₂. Which holds more moles, Zee?
- Neither: n = PV ÷ (RT) is the same for both
- The CO₂, since it is heavier
- The O₂, since it is lighter
Which change doubles a gas's volume at fixed pressure, Ari?
- Doubling its kelvin temperature
- Halving its kelvin temperature
- Doubling its Celsius temperature