The temperature of a gas in a closed container is 27° C . If the temperature is raised to 327° C, the pressure exerted is

Question

The temperature of a gas in a closed container is 27° C . If the temperature is raised to 327° C, the pressure exerted is (A) reduced to half (B) doubled (C) reduced to one third (D) cannot be predicted

Tardigrade Admin · Accepted Answer

(p1/T1)=(p2/T2) Given, T1=27+273=300 text K T2=327+273=600 text K So, (p1/300)=(p2/600) ∴ P2=(600/300)p1=2p1 ie, pressure becomes doubled.

Q. The temperature of a gas in a closed container is $27^{\circ} C$ . If the temperature is raised to $327^{\circ} C,$ the pressure exerted is

reduced to half

doubled

reduced to one third

cannot be predicted

$\frac{p _{1}}{T _{1}} = \frac{p _{2}}{T _{2}}$ Given, $T_{1} = 27 + 273 = 300 K$ $T_{2} = 327 + 273 = 600 K$ So, $\frac{p _{1}}{300} = \frac{p _{2}}{600}$ $∴$ $P_{2} = \frac{600}{300} p_{1} = 2 p_{1}$ ie, pressure becomes doubled.

Q. The temperature of a gas in a closed container is 27∘C . If the temperature is raised to 327∘C, the pressure exerted is