The temperature of a gas at 1.00 atm and 8.00$\degree$C is increased to 20.0$\degree$C, resulting in a change of pressure. What is the new pressure?
A) 0.400 atm.
B) 0.967 atm.
C) 1.00 atm.
D) 1.04 atm.
E) 2.50 atm.

Question

Quizplus · Accepted Answer

First, we need to convert the temperatures to absolute temperature using the Kelvin scale:
Initial temperature = (8.00 + 273) K = 281 K
Final temperature = (20.0 + 273) K = 293 K

Using the combined gas law: P1V1/T1 = P2V2/T2
Since the volume is constant, we can simplify the equation to: P1/T1 = P2/T2

Substituting the values:
P1 = 1.00 atm
T1 = 281 K
T2 = 293 K

P2 = (P1/T1) x T2
P2 = (1.00 atm/281 K) x 293 K
P2 = 1.04 atm

Therefore, the new pressure is 1.04 atm (choice D).

The Temperature of a Gas at 1 °\degree° C Is Increased to 20

The Temperature of a Gas at 1 $\degree$ C Is Increased to 20