If 6.15 L of CH4 undergoes complete combustion at 943.97 mm Hg and 83.47ºC, how many grams of H2O is formed?CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

Question

If 6.15 L of CH4 undergoes complete combustion at 943.97 mm Hg and 83.47ºC, how many grams of H2O is formed?CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

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Solution 1

To solve this problem, we need to use the ideal gas law and stoichiometry. Here are the steps:

Convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15. So, 83.47ºC = 83.47 + 273.15 = 356.62 K.
Convert the pressure from mm Hg to atm. The conv Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.

Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
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Similar Questions

If 6.15 L of CH4 undergoes complete combustion at 943.97 mm Hg and 83.47ºC, how many grams of H2O is formed?CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

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