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Problem: Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.How many moles of water can you make?

🤓 Based on our data, we think this question is relevant for Professor Pierino's class at Colorado School of Mines.

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Reaction involved (combustion): CH4 + 2O2 → CO2 + 2H2O

We shall determine the moles of water produced by each reactant. The reactant that produces the least number of moles of water is the limiting reactant and shall produce the theoretical number of moles of water.

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Problem Details

Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g of oxygen (O2) gas and then ignite the mixture. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel.

How many moles of water can you make?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Pierino's class at Colorado School of Mines.