What is the final pressure of the gas in the following problem?
If I have 17 Liters of gas at a temperature of 67°C and a pressure of 88.89 atm. What will be the pressure of the gas if I raise the temperature to 94°C and decrease the volume to 12 Liters?
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The problem given is that initially there are 17 L of gas at 67 degree Celsius and the pressure is 88.89 atm. We need to determine the pressure if the temperature is raised to 94 degree Celsius and the volume is decreased to 12 L.
We use the ideal gas law, which gives the relation between pressure, temperature and volume as P*V = n*R*T, where P is the pressure, V is the volume, n is the amount of substance, R is a constant and T is the temperature.
Let's rewrite the relation as n*R = P*V/T, we now have constants on one side and the variables on the other side.
Substituting the values given:
17*88.89 / 67 = P*12 / 94
=> P = 17*88.89*94/(12*67)
=> P = 176.67 atm.
When the conditions are altered the pressure of the gas increases to 176.67 atm.
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