How many liters of CH4 (g), measured at 22.6 ∘C and 768 mmHg, must be burned to provide the heat needed to vaporize 3.82 L of water at 100 ∘C? ΔcombH=-8.90*102kJmol-1 CH4. For H2O (l) at 100 ∘C, d=0.958gcm-3 and ΔvapH=40.7kJmol-1.

Express your answer in liters to three significant figures.

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22 January, 12:05

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Brent · Answer 1

For H2O (l) at 100 ∘C, d=0.958gcm-3 and ΔvapH=40.7kJmol-1.

How many liters of CH4 (g), measured at 22.6 ∘C and 768 mmHg, must be burned to provide the heat needed to vaporize 3.82 L of water at 100 ∘C? ΔcombH=-8.90*102kJmol-1 CH4. For H2O (l) at 100 ∘C, d=0.958gcm-3 and ΔvapH=40.7kJmol-1.Express your answer in liters to three significant figures.