A 0.316 mol sample of nitrogen gas, N2(g), is placed in a 4.00 L container at 315K
What is the pressure, in Torr, of the nitrogen gas?
Torr

1550.8

Explanation:

This is the ideal gas equation:

PV=nRT

We can rearrange the ideal gas equation to solve for the pressure of the nitrogen gas.

P=nRT/ V

We can find the pressure of the nitrogen gas by plugging in the values for the moles of gas, temperature, and volume. Since we want the pressure in units of Torr we use the R value62.36358L Torr K−1 mol-1

P=nRT/ V

(0.316 mol )(62.36358 L*Torr/K*mol)(315 K) / 4.00 L =1550 Torr

The correct answer is 1550

the answer would be c

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