A6.34l sample of hydrogen gas exerts a pressure of 1.52 atm at 298k. what temperature would be required for it to have a volume of 4.98l and a pressure of 0.720 atm?

There is a temperature of 111 K required.

Explanation:

Step 1: Data given

Volume of hydrogen gas = 6.34 L

Pressure = 1.52 atm at 298 K

The volume of the gas at a pressure of 0.720 atm is 4.98 L

Step 2:

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

⇒ with P1 = the pressure of the hydrogen gas = 1.52 atm

⇒ with V1 = the volume of the hydrogen gas = 6.34 L

⇒ with T1 = the temperature of the hydrogen gas = 298 K

⇒ with P2 = the changed pressure of the gas = 0.720 atm

⇒ with V2 = the changed volume of the gas = 4.98 L

⇒ with T2= the temperature of the gas at 0.720 atm and 4.98L

(1.52*6.34)/298 = (0.720*4.98)/T2

0.0323 = 3.5856/T2

T2 = 110.88 K ≈111K

There is a temperature of 111 K required.

"record the time to complete a chemical reaction" would most likely be part of a lab procedure.

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