Question

1- A sample of carbon dioxide gas at a pressure of 1.03 atm and a temperature of 210 °C, occupies a volume of 546 mL. If the gas is cooled at constant pressure until its volume is 443 mL, the temperature of the gas sample will be ______ °C.

2- A sample of nitrogen gas at a pressure of 831 mm Hg and a temperature of 81 °C, occupies a volume of 6.66 liters. If the gas is heated at constant pressure to a temperature of 107 °C, the volume of the gas sample will be ______ L.

3- A sample of gas contains 0.1800 mol of C₂H₄(g) and 0.1800 mol of H₂O₂(g) and occupies a volume of 11.7 L. The following reaction takes place:

C₂H₄(g) + H₂O₂(g) = CH₂OHCH₂OH(g)

Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
______ L

4- A sample of helium gas at a pressure of 0.887 atm and a temperature of 28.3 °C, occupies a volume of 458 mL. If the gas is allowed to expand at constant temperature until its pressure is 0.681 atm, the volume of the gas sample will be ____mL.

5- A sample of hydrogen gas at a pressure of 1.04 atm and a temperature of 20.9 °C, occupies a volume of 15.8 liters. If the gas is allowed to expand at constant temperature to a volume of 24.3 liters, the pressure of the gas sample will be _____ atm

Answer 1

1) According to Charless law, volume of the gasis directly proporti onal to absolute temperature at constant pressure Voc T V constant For twogasses Initi al volume of the gas, 546 mL = 483 K Initi al temperature of the the gas, T 210°C+273 Final temperature of the gas Final volume of the of the the gas, V = 443 mL According to Charlesslaw Final temperature of gas 443 mL = 483 K 546 mL = 119° C 392 K -273