a gas exerts a pressure of 125.0 mm hg in a container with an unknown volume. the gas exerts a pressure of…

a gas exerts a pressure of 125.0 mm hg in a container with an unknown volume. the gas exerts a pressure of 145 mm hg when transferred to a container with a volume of 0.4650 l. what is the initial volume of the gas? v = ? l assume that the number of moles and the temperature remain constant.

a gas exerts a pressure of 125.0 mm hg in a container with an unknown volume. the gas exerts a pressure of 145 mm hg when transferred to a container with a volume of 0.4650 l. what is the initial volume of the gas? v = ? l assume that the number of moles and the temperature remain constant.

Answer

Explanation:

Step1: Identify the relevant law

Boyle's law states $P_1V_1 = P_2V_2$ for a gas at constant temperature and number of moles.

Step2: Assign values

Let $P_1 = 125.0\ mmHg$, $V_1$ be the unknown initial - volume, $P_2=145\ mmHg$, and $V_2 = 0.4650\ L$.

Step3: Rearrange the formula to solve for $V_1$

$V_1=\frac{P_2V_2}{P_1}$.

Step4: Substitute the values

$V_1=\frac{145\ mmHg\times0.4650\ L}{125.0\ mmHg}$. $V_1=\frac{67.425}{125.0}\ L$. $V_1 = 0.5394\ L$.

Answer:

$0.5394$