Question

Consider 4.70 L of a gas at 365 mmHg and 20. ∘C . If the container is compressed to 2.00 L and the temperature is increased to 36 ∘C , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder.

Answer 1

To find the new pressure inside the container, we can use the combined gas law formula P1V1/T1 = P2V2/T2. By substituting the given values, we find that the new pressure, P2, is approximately 421.53 mmHg.

Step-by-step explanation:

The question asks for the new pressure, P2, inside the container after it is compressed to 2.00 L and the temperature is increased to 36 °C, assuming no change in the amount of gas. To solve this, we can use the combined gas law formula, which states P1V1/T1 = P2V2/T2. We are given that the initial pressure, P1, is 365 mmHg, the initial volume, V1, is 4.70 L, the initial temperature, T1, is 20 °C, the final volume, V2, is 2.00 L, and the final temperature, T2, is 36 °C.

First, we need to convert the temperatures to Kelvin by adding 273.15. So, T1 = 20 °C + 273.15 = 293.15 K and T2 = 36 °C + 273.15 = 309.15 K. Now we can substitute the values into the combined gas law formula:

365 mmHg * 4.70 L / 293.15 K = P2 * 2.00 L / 309.15 K

Solving this equation gives us the final pressure, P2, which is approximately 421.53 mmHg.