The reaction in question will be carried out in a calorimeter. The volume of the

Question

The reaction in question will be carried out in a calorimeter. The volume of the chamber inside is 2.00 leaders. Experiment starts by evacuating the chamber to 0.00 kPa. Then oxygen gas is filled into the chamber till pressure is 200. kPa. The hydrogen gas is filled into the same chamber until total pressure is 400. kPa. The oxygen and hydrogen mixture is ignited by spark with 3.00 kJ of energy. Calculate the total pressure inside the chamber after reaction. The capacity of this calorimeter is 944.12J/K. The initial temperature is 25 degree celsius.

The reaction in question will be carried out in a calorimeter. The volume of the chamber inside is 2.00 leaders. Experiment starts by evacuating the chamber to 0.00 kPa. Then oxygen gas is filled into the chamber till pressure is 200. kPa. The hydrogen gas is filled into the same chamber until total pressure is 400. kPa. The oxygen and hydrogen mixture is ignited by spark with 3.00 kJ of energy. Calculate the total pressure inside the chamber after reaction. The capacity of this calorimeter is 944.12J/K. The initial temperature is 25 degree celsius.

Explanation / Answer

H2(g) + (1/2)O2  -----> H2O(l)

As per the balanced reaction H2 & O2 reacts in the molar ratio of 1:0.5

Now, initial moles of oxygen = (P*V)/(R*T) = (200000*2/101325)/(0.0821*298) = 0.16 = Moles of Hydrogen gas

Now, moles of hydrogen left unreacted = 0.16/2 = 0.08

Rise in temperature of the calorimeter = energy added/calorimeter capacity = 3000/944.12 = 3.18

Thus, final temperature of the calorimeter = 28.18 0C

Thus, final pressure = moles of H2 left unreacted*R*final temperature/V = 0.08*0.0821*301.18/2 = 0.989 atm = 100.22 kPa

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