To** calculate new pressure**, we use** Gay-Lussac's Law**:

$\overline{)\frac{{\mathbf{P}}_{\mathbf{1}}}{{\mathbf{T}}_{\mathbf{1}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{2}}}{{\mathbf{T}}_{\mathbf{2}}}}$

Rearranging to solve for P_{2}:

$\overline{){{\mathbf{P}}}_{{\mathbf{2}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{1}}}{{\mathbf{T}}_{\mathbf{1}}}\left({\mathbf{T}}_{\mathbf{2}}\right)}$

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 306 K, but the container does not expand. What will the new pressure be?

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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law Derivations concept. You can view video lessons to learn The Ideal Gas Law Derivations. Or if you need more The Ideal Gas Law Derivations practice, you can also practice The Ideal Gas Law Derivations practice problems.