Question
A sample of nitrogen has a volume of 1.75 L, a pressure of 2.00 atm, and a temperature of 35 °C. What is the new temperature, if the new volume is 2.45 L and the new pressure is 1.32 atm?
Answers
Answered by
GPT 3.5
To solve this problem, we can use the combined gas law formula:
(P1)(V1) / (T1) = (P2)(V2) / (T2)
Where:
P1 = initial pressure = 2.00 atm
V1 = initial volume = 1.75 L
T1 = initial temperature = 35 °C = 308 K
P2 = final pressure = 1.32 atm
V2 = final volume = 2.45 L
T2 = final temperature
Now, plug in the values into the formula:
(2.00 atm)(1.75 L) / (308 K) = (1.32 atm)(2.45 L) / (T2)
Solving for T2:
(3.50 atm*L) / (308 K) = (3.24 atm*L) / (T2)
T2 = (3.24 atm*L) / (3.50 atm) * (308 K)
T2 = 284.16 K
Therefore, the new temperature is 284.16 K.
(P1)(V1) / (T1) = (P2)(V2) / (T2)
Where:
P1 = initial pressure = 2.00 atm
V1 = initial volume = 1.75 L
T1 = initial temperature = 35 °C = 308 K
P2 = final pressure = 1.32 atm
V2 = final volume = 2.45 L
T2 = final temperature
Now, plug in the values into the formula:
(2.00 atm)(1.75 L) / (308 K) = (1.32 atm)(2.45 L) / (T2)
Solving for T2:
(3.50 atm*L) / (308 K) = (3.24 atm*L) / (T2)
T2 = (3.24 atm*L) / (3.50 atm) * (308 K)
T2 = 284.16 K
Therefore, the new temperature is 284.16 K.