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.

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.