The constant-volume tank contains 1 kmol of methane (ch4) gas and 3 kmol of o2 at 25°c and 1 atm. the contents of the tank are ignited, and the methane gas burns completely. if the final temperature is 1000 k, determine the final pressure in the tank.
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The balanced combustion reaction is
CH₄ + 3O₂ ⇒ CO₂ + 2H₂O + O₂
Number of moles of reactants , n₁ = 1 + 3 = 4
number of moles of products , n₂ = 1 + 2 + 1 = 4
We know one thing , at 1000K water exists an gas phase , so using ideal gas equation relation for both reactant and product , the final pressure in the rank is determined to be :
P₁V₁/n₁T₁ = P₂V₂/n₂T₂
P₁ = 1atm , P₂ = ? , v₁ = V₂ = V [ because reaction occurs in tank ]
n₁ = n₂ = 4 , T₁ = 25° = 298K and T₂ = 1000K
so, 1 × V/4 × 298 = P₂ × V/4 × 1000
P₂ = 1000/298 = 3.36 atm
Hence, final pressure is 3.36 atm
CH₄ + 3O₂ ⇒ CO₂ + 2H₂O + O₂
Number of moles of reactants , n₁ = 1 + 3 = 4
number of moles of products , n₂ = 1 + 2 + 1 = 4
We know one thing , at 1000K water exists an gas phase , so using ideal gas equation relation for both reactant and product , the final pressure in the rank is determined to be :
P₁V₁/n₁T₁ = P₂V₂/n₂T₂
P₁ = 1atm , P₂ = ? , v₁ = V₂ = V [ because reaction occurs in tank ]
n₁ = n₂ = 4 , T₁ = 25° = 298K and T₂ = 1000K
so, 1 × V/4 × 298 = P₂ × V/4 × 1000
P₂ = 1000/298 = 3.36 atm
Hence, final pressure is 3.36 atm
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