To be able to solve this, one important statement should be present which is that this gas is ideal. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant volume and number of moles of the gas the ratio of T and P is equal to some constant. At another set of condition, the constant is still the same. Calculations are as follows:
T1/P1 = T2/P2
P2 = T2 x P1 / T1
P2 = 311 K (1 atm) / 273 K
P2 = 1.14 atm
Therefore, the increase in temperature from 273 K to 311 K at a constant volume lead to an increase of the pressure to 1.14 atm.
Answer:
The required variables are P,V
Explanation:
Since temperature increases, it must be included in your formula. Since you are solving for pressure, it must also be included. However, since the number of moles and the volume remain the same, they can be excluded.
