# What amount of heat will be released during the combustion of 100 liters of hydrogen

July 26, 2021 | education

| **What amount of heat will be released during the combustion of 100 liters of hydrogen, taken under normal conditions? Thermochemical equation of the reaction: 2H2 (G) + O2 (G) = 2H2O (G) +484 KJ**

Answer: Q = 1079.32 kJ.

Explanation of the solution to the problem: to solve this problem, you first need to find the amount of hydrogen substance (the volume of hydrogen is divided by the molar volume (22.4 l / mol)):

n = V / Vm = 100 / 22.4 = 4.46 mol.

Now we need to make a proportion: from the chemical reaction equation, we know that when two moles of hydrogen are burned, 484 kJ of heat is released, which means that when 4.46 moles of hydrogen are burned, Q of heat is released:

2 mol – 484 kJ;

4.46 mol – Q kJ.

Hence Q = 4.46 * 484/2 = 1079.32 kJ.

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