Agas in a rigid container at 25°c has a pressure of 0.96 atm. a change in temperature causes the pressure to increase to 1.25 atm. what is the new temperature of the gas?

The new temperature  of the gas is  388.02 k  or 115.02°c

 calculation

The  new temperature  is calculated  using Gay Lussac's   formula

That is P₁/T₁ = P₂/T₂

where;

P₁  = 0.96 atm

T₁ = 25°c into kelvin   = 25 +273  =298 k

P₂= 1.25 atm

T₂ =  ?  k

make T₂ the subject of the formula

T₂ = P₂T₁/P₁

 = (1.25 atm x 298 k) / 0.96 atm  =  388.02 K   or  388.02 -273 =115.02°c

the answer is the

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.