Question

A gas in a closed container has a pressure of 1.20 atm at a temperature of 308 K. If the pressure in the container is increased to 2.10 atm, what is the new temperature?



Use the sample problem below and follow the 5 steps to help you solve the problem you were given.



a
539 K
b
370 K
c
176 K
d
122 K

Answer 1

To solve this problem using the 5 steps, we can use the combined gas law equation, which is:

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

Step 1: Write down the known values
P1 = 1.20 atm
T1 = 308 K
P2 = 2.10 atm

Step 2: Determine the unknown value you need to find
We need to find T2, the new temperature.

Step 3: Rearrange the equation to solve for the unknown value
(T2) = (P2 x V2 x T1) / (P1 x V1)

Step 4: Substitute the known values into the rearranged equation
(T2) = (2.10 atm x T1) / (1.20 atm)

Step 5: Calculate the unknown value
(T2) = (2.10 atm x 308 K) / (1.20 atm)
(T2) = 539 K

Therefore, the new temperature is 539 K. The correct answer is a) 539 K.