One mole of an ideal gas is sealed in a 22.4-l container at a pressure of 1 atm and a temperature of 273 k. the temperature is then increased to 311 k, but the container does not expand. what will the new pressure be? part a the most appropriate formula for solving this problem includes only which variables? enter the required variables, separated by commas (e. g., p, v, t).

Question

Chemistry

Kolten Townsend

14 September, 09:51

One mole of an ideal gas is sealed in a 22.4-l container at a pressure of 1 atm and a temperature of 273 k. the temperature is then increased to 311 k, but the container does not expand. what will the new pressure be? part a the most appropriate formula for solving this problem includes only which variables? enter the required variables, separated by commas (e. g., p, v, t).

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Pebbles · Answer 1

To be able to solve this, one important statement should be present which is that this gas is ideal. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant volume and number of moles of the gas the ratio of T and P is equal to some constant. At another set of condition, the constant is still the same. Calculations are as follows:

T1/P1 = T2/P2

P2 = T2 x P1 / T1

P2 = 311 K (1 atm) / 273 K

P2 = 1.14 atm

Therefore, the increase in temperature from 273 K to 311 K at a constant volume lead to an increase of the pressure to 1.14 atm.