Question
A gas in a closed container has a pressure of 6.40 atm at a temperature of 230 K. If the pressure in the container is decreased to 5.30 atm, what is the new temperature? a 890 K b 278 K c 83 K d 190 K
Answers
GPT 3.5
To solve this problem, we can use the combined gas law, which states: P1V1/T1 = P2V2/T2, where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures.
Given:
P1 = 6.40 atm
T1 = 230 K
P2 = 5.30 atm
Let's assume the volume remains constant, so V1 = V2. We can rewrite the equation as:
P1/T1 = P2/T2
Substituting the given values, we have:
6.40 atm / 230 K = 5.30 atm / T2
Simplifying the equation, we get:
6.40T2 = 5.30 * 230
T2 = (5.30 * 230) / 6.40
Calculating the right side of the equation, we have:
T2 = 191.0625 ≈ 191 K
Therefore, the new temperature is approximately 191 K, which is closest to 190 K (option d).
Given:
P1 = 6.40 atm
T1 = 230 K
P2 = 5.30 atm
Let's assume the volume remains constant, so V1 = V2. We can rewrite the equation as:
P1/T1 = P2/T2
Substituting the given values, we have:
6.40 atm / 230 K = 5.30 atm / T2
Simplifying the equation, we get:
6.40T2 = 5.30 * 230
T2 = (5.30 * 230) / 6.40
Calculating the right side of the equation, we have:
T2 = 191.0625 ≈ 191 K
Therefore, the new temperature is approximately 191 K, which is closest to 190 K (option d).