3 years ago

At 393 K, the pressure of a sample of nitrogen is 1.07 atm. What will the pressure be at 478 K, assuming constant volume?

Chemistry

1 answer:

True [87]3 years ago

7 0

Answer:

About 1.301 atm

Explanation:

The formula that you should is PV=nRT, where P stands for pressure, V stands for volume, n stands for the number of moles, R stands for the universal gas constant, and T stands for temperature in Kelvin. Since the volume, number of moles, and universal gas constant don't change, you don't need to worry about them.

1.07V=393nR

PV=498nR

P=1.301 atm. Hope this helps!

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