Q. 8.19 - An Introduction to General, Organic, and Biological Chemistry

Question

A sample of Ar gas has a volume of 5.40 L with an unknown pressure. The gas has a volume of 9.73 L when the pressure is 3.62 atm, with no change in temperature or amount of gas. What was the initial pressure, in atmospheres, of the gas?

Step-by-Step Solution

Answer

The initial pressure of the gas was  $6.52 atm$.

Step 1: Given information

We need to find the initial pressure of the gas

Step 2: Explanation

We can apply Boyle's law as the temperature is constant 

$P1V1=P2V2$

Now,

$V1=5.40 L$

$P2=3.62 atm$

$V2=9.73 L$

Substituting the values we get,

$P1=\frac{3.62 atm\times 9.73 L}{5.40 L}=6.52 atm$

So the initial pressure of the gas was $6.52 atm$