Question

Hydrogen gas at a temperature of 22.0°C that is confined in a 5.00L cylinder exerts a pressure of 4.20atm. If the gas is released into a 10.0L reaction vessel at a temperature of 33.6°C, what will be the pressure inside the reaction vessel?

Answer 1

The pressure inside the reaction vessel is 2.18 atm

Step-by-step explanation:

Step 1: Data given

The temperature = 22.0 °C = 295.15 K

Pressure = 4.20 atm

Volume = 5.0 L

Volume increased to 10.0 L

Temperature increased to 33.6 °C = 306.75K

Step 2: Calculate the new pressure

P1 * V1 / T1 = P2*V2 / T2

⇒with P1 = the initial pressure = 4.20 atm

⇒with V1 = the initial volume = 5.0 L

⇒with T1 = the initial temperature = 295.15 K

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 10.0L

⇒with T2 = the increased temperature = 306.75 K

(4.20 atm * 5.0 L) / 295.15 K = ( P2 * 10.0 L ) / 306.75 K

P2 = (4.20 * 5.0 L * 306.75 K) / (295.15 K * 10.0 L)

P2 = 2.18 atm

The pressure inside the reaction vessel is 2.18 atm

Answer 2

THE NEW PRESSURE WHEN THE GAS IS RELEASED INTO A 10 L REACTION VESSEL AND AT 33.6 °C TEMPERATURE IS 2.18 atm.

Step-by-step explanation:

The general gas equation will be used to calculate the new pressure.

P1V1 /T1 = P2 V2 / T2

P1 = 4.20 atm

V1 = 5 L = 5 dm3

T1 = 22°C = 22 + 273 K = 295 K

V2 = 10 L = 10 dm3

T2 = 33.6 °C = 33.6 + 273 K = 306.6 K

P2 =?

Rearranging the formula and making P2 the subject of the equation, we have;

P2 = P1V1 T2 / T1 V2

P2 = 4.2 * 5 * 306.6 / 295 * 10

P2 = 6438.6 / 2950

P2 = 2.18 atm.

So therefore, the pressure inside the reaction vessel when the gas is released into a 10 L reaction vessel and at a temperature of 33.6 °C is 2.18 atm.