Answer:
New pressure is 0.534 atm
Explanation:
Given:
Initial volume of the gas, V₁ = 250 mL
Initial pressure of the gas, P₁ = 1.00 atm
Initial temperature of the gas, T₁ = 20° C = 293 K
Final volume of the gas, V₂ = 500 mL
Final pressure of the gas = P₂
Final temperature of the gas, T₁ = 40° C = 313 K
now,
we know for a gas
PV = nRT
where,
n is the moles
R is the ideal gas constant
also, for a constant gas
we have
(P₁V₁/T₁) = (P₂V₂/T₂)
on substituting the values in the above equation, we get
(1.00 × 250)/293 = (P₂ × 500)/313
or
P₂ = 0.534 atm
Hence, the new pressure is 0.534 atm
