Question

fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C

Answer 1

Answer:

846.45 torr

Explanation:

According to Boyle's Law

P1V1=P2V2

(10)(667)=(7.88)(P2)

P2=846.45torr

Answer 2

Answer: The final pressure of the gas is 846.44 torr

Explanation:

To calculate the new volume, we use the equation given by Boyle's law. This law states that pressure is inversely proportional to the volume of the gas at constant temperature.

The equation given by this law is:

$P_1V_1=P_2V_2$

where,

$P_1\text{ and }V_1$ are initial pressure and volume of the gas.

$P_2\text{ and }V_2$ are final pressure and volume of the gas

We are given:

$P_1=667torr\\V_1=10.0L\\P_2=?torr\\V_2=7.88L$

Putting values in above equation, we get:

$667torr\times 10.0L=P_2\times 7.88\\\\P_2=\frac{667\times 10.0}{7.88}=846.44torr$

Hence, the final pressure of the gas is 846.44 torr