Consider the conversion of methane to acetylene and hydrogen gas shown in the unbalanced reaction below:CH₄ $\rightarrow$C₂H₂ + H₂What is the final pressure in a 100 L reaction vessel following the conversion of 323 g of methane to acetylene and hydrogen gases at 1725°C?

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The balanced reaction is 2CH₄ → C₂H₂ + 3H₂. Calculate moles of CH₄: 323 g / 16.04 g/mol = 20.14 mol. From stoichiometry, 20.14 mol CH₄ produces 10.07 mol C₂H₂ and 30.21 mol H₂, totaling 40.28 mol of gas. Using the ideal gas law (PV=nRT), with R=0.08314 L·bar/mol·K and T=1998 K (1725°C + 273), P = (40.28 mol)(0.08314 L·bar/mol·K)(1998 K) / 100 L = 67.0 bar.

Consider the Conversion of Methane to Acetylene and Hydrogen Gas →\rightarrow→

Consider the Conversion of Methane to Acetylene and Hydrogen Gas $\rightarrow$