Part 1) A sample of krypton gas at a pressure of 0.962 atm and a temperature of 21.0 °C, occupies a volume of 889 mL. If the gas is compressed at constant temperature until its pressure is 1.45 atm, the volume of the gas sample will be mL

part 2) A sample of nitrogen gas at a pressure of 555.1 mm Hg and a temperature of 24.7 °C, occupies a volume of 12.5 liters. If the gas is allowed to expand at constant temperature to a volume of 20.2 liters, the pressure of the gas sample, in atmospheres, will be atm.

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answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

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