Question

One mole of oxygen gas is at a pressure of 6.30 atm and a temperature of 24.0°C.

If the gas is heated at constant volume until the pressure triples, what is the final temperature?
°C ?

Answer 1

To find the final temperature, we can use the combined gas law. Using the given initial and final conditions, we can plug the values into the equation and solve for the final temperature. The final temperature can be calculated in Kelvin and then converted back to Celsius by subtracting 273.15.

Step-by-step explanation:

To solve this problem, we can use the combined gas law, which relates the initial and final temperatures, pressures, and volumes of a gas sample. The combined gas law equation is:

(P1 * V1) / T1 = (P2 * V2) / T2

We are given that the initial temperature (T1) is 24.0°C, the initial pressure (P1) is 6.30 atm, and the initial volume (V1) is constant. We want to find the final temperature (T2) when the pressure (P2) triples. Let's represent the final pressure as 1 atm * 3 = 3 atm and the final volume as V1. We can plug these values into the combined gas law equation to solve for T2: (6.30 atm * V1) / (24.0 + 273.15 K) = (3 atm * V1) / T2

Cross-multiplying and then solving for T2, we get:

T2 = (3 * 24.0 + 273.15 K) / (6.30)

Calculating this expression will give us the final temperature in Kelvin. To convert it back to Celsius, subtract 273.15 from the result.