Question

a sealed container holds a gas at a pressure of 1.5 atm and a temperature of 300 k. if the temperature is increased to 450 k while the volume remains constant, what will be the new pressure of the gas? the new pressure would be select one select one

Explanation:

Step1: Identify the gas law

Since the volume is constant, use Gay - Lussac's law: $\frac{P_1}{T_1}=\frac{P_2}{T_2}$.

Step2: Substitute the given values

Given $P_1 = 1.5$ atm, $T_1=300$ K, $T_2 = 450$ K.
We can solve for $P_2$: $P_2=\frac{P_1\times T_2}{T_1}$.
Substitute the values: $P_2=\frac{1.5\times450}{300}$.

Step3: Calculate the new pressure

$P_2=\frac{675}{300}=2.25$ atm.

Answer:

$2.25$ atm