Afixed 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. a. 846 torrb. 526 torrc. 0.118 torrd. 1.11 torre. 5.26 × 104 torr

The pressure, when the volume is reduced to 7.88L, is 846 torr (option A)

Explanation:

Step 1: Data given

The temperature of a gas = 25.0°C

AT 25 °C the gas occupies a volume of 10.0L and a pressure of 667 torr.

The volume reduces to 7.88 L but the temperature stays constant.

Step 2: Boyle's law

(P1*V1)/T1 = (P2*V2)/T2

 ⇒ Since the temperature stays constant, we can simplify to:

P1*V1 = P2*V2

⇒ with P1 = the initial pressure 667 torr

⇒ with V1 = the initial volume = 10.0 L

⇒ with P2 = the final pressure = TO BE DETERMINED

⇒ with V2 = the final volume = 7.88L

P2 = (P1*V1)/V2

P2 = (667*10.0)/7.88

P2 = 846 torr

The pressure, when the volume is reduced to 7.88L, is 846 torr (option A)

idk i’m struggling too

the answer is d. 74.02