A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm.What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?
A) 10.2 atm
B) 9.83 atm
C) 15.3 atm
D) 6.53 atm
E) 1.05 atm

Question

Quizplus · Accepted Answer

The correct answer can be found using the combined gas law: $P_1V_1/T_1 = P_2V_2/T_2$. Solving for $P_2$, we get $P_2 = (P_1V_1T_2)/(T_1V_2)$. Plugging in the given values: $P_2 = (2.20 \, \text{atm} \times 859 \, \text{mL} \times 815 \, \text{K}) / (565 \, \text{K} \times 268 \, \text{mL})$, which calculates to approximately 10.2 atm.

A Sample of Gas Initially Has a Volume of 859