Answer: Volume of hydrogen gas at 117⁰C is 27.27 mL .
Explanation: Pressure is constant , thus the process is isobaric. Here Charles law is valid , Charles law state that at constant pressure the volume of fixed amount of gas is directly proportional to the absolute temperature of the gas.
Equation :- at constant pressure P ,
V ∝ T ⇒ V = nT ,
here n is the proportionality constant and depends on the value of pressure and units .
The above given law can also be written as, V/T = constant or
V₁/T₁ = V₂/T₂ ( equation 1)
V₁ = initial volume of H₂( hydrogen ) gas = 20mL
T₁ = initial temperature of H₂ gas = 13⁰ C = 273+13 = 286 K
V₂ = final volume of gas
T₂= final temperature of gas = 117⁰ C = 273+117 = 390K
Putting the values in equation 1
20/ 286 = V₂/390 ⇒ V₂ = 20 × 390 / 286 = 7800/286
V₂ = 27.27 mL
Hence the volume of H₂ gas at 117⁰C is 27.27 mL
Here it should be noted that the H₂ gas is treated as ideal gas, this is an assumption that is taken for the sake of calculations.
Answers & Comments
Answer: Volume of hydrogen gas at 117⁰C is 27.27 mL .
Explanation: Pressure is constant , thus the process is isobaric. Here Charles law is valid , Charles law state that at constant pressure the volume of fixed amount of gas is directly proportional to the absolute temperature of the gas.
Equation :- at constant pressure P ,
V ∝ T ⇒ V = nT ,
here n is the proportionality constant and depends on the value of pressure and units .
The above given law can also be written as, V/T = constant or
V₁/T₁ = V₂/T₂ ( equation 1)
V₁ = initial volume of H₂( hydrogen ) gas = 20mL
T₁ = initial temperature of H₂ gas = 13⁰ C = 273+13 = 286 K
V₂ = final volume of gas
T₂= final temperature of gas = 117⁰ C = 273+117 = 390K
Putting the values in equation 1
20/ 286 = V₂/390 ⇒ V₂ = 20 × 390 / 286 = 7800/286
V₂ = 27.27 mL
Hence the volume of H₂ gas at 117⁰C is 27.27 mL
Here it should be noted that the H₂ gas is treated as ideal gas, this is an assumption that is taken for the sake of calculations.