The temperature of a gas at 1.00 atm and 8.00 °C is increased to 20.0 °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

The new pressure can be calculated using the ideal gas law, assuming the volume and the amount of gas remain constant. The relationship between pressure and temperature for a gas is given by $P_1/T_1 = P_2/T_2$, where $P_1$ and $P_2$ are the initial and final pressures, and $T_1$ and $T_2$ are the initial and final temperatures in Kelvin. Converting the temperatures to Kelvin: $T_1 = 8.00 + 273.15 = 281.15$ K and $T_2 = 20.0 + 273.15 = 293.15$ K. Substituting the given values and solving for $P_2$, we get $P_2 = P_1 \times (T_2/T_1) = 1.00 \times (293.15/281.15) \approx 1.04$ atm.

The Temperature of a Gas at 1