Question

The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 88 ∘C ?

Answer 1

2.58 atm

Step-by-step explanation:

P1 = 2.1 atm

T1 = 21 °C = 294 K

T2 = 88 °C = 361 K

P2 = ?

By using the gas laws

P / T = constant keeping the volume constant.

P1 / T1 = P2 / T2

2.10 / 294 = P2 / 361

P2 = 2.58 atm

Thus, the pressure becomes 2.58 atm.

Answer 2

2.57832 atm

Step-by-step explanation:

`P_1` = Initial pressure = 2.1 atm

`P_2` = Fianl pressure

`T_1` = Initial Temperature = (21+273.15) K

`T_2` = Final Temperature = (88+273.15) K

From Gay-Lussacs law we have

`(P_1)/(T_1)=(P_2)/(T_2)\\\Rightarrow P_2=(P_1* T_2)/(T_1)\\\Rightarrow P_2=(2.1* (88+273.15))/(21+273.15)\\\Rightarrow P_2=2.57832\ atm`

The final pressure would be 2.57832 atm