Question

help please chemistry

at constant volume, the pressure in a cylinder of gas is 345 kPa at a temp of 27 Celsius what would be the pressure of this Cylinder of gas if the temp changes in hot sun to 47 C°

how do I solve and what's answer​
will give brainliest

Answer 1

The Ideal Gas Law states that PV=nRT where P is pressure, V is volume, n is number of molecules, R is the gas constant and T is the temp.

As number of molecules does not change and volume of cylinder does not change, we move the constants to one side: P/T=nR/V=constant.

We get P1/T1=P2/T2

Temp should be in K so T1=27C+273=300K

T2=47C+273=320K

P2=T2*P1/T1=320*345/300

=368kPa

Answer 2

Gay-Lussac's Law states that under constant volume, pressure of a gas is directly proportional to its absolute temp

absolute temp1 = 273+27 = 300K

absolute temp2 = 273+47 = 320K

new pressure = old pressure x 320/300 = 345 x 320/300

= 368 kPa