# What mass of natural gas (CH4) must you burn to emit 271kJ of heat? CH4(g)+2O2(g)-->CO2(g)+2H2O(l) Delta H rxn = -802.3 kJ

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Apr 7, 2015

$\Delta {H}_{r x n}$ shows the amount of enerjy (heat) emitted or absorbed when 1 mole of reactant is used. Which means for this reaction when 1 mole of CH4 burned 802 kJ heat was released.
1 mole of CH4 is 16 grams.

So if we know that for 802 kJ heat release 16 grams of methane is needed then we can find the amount of methane needed to be burnt for 271 kJ heat to be released:

$271 k J \cdot \left(\frac{16 g C {H}_{4}}{802 k J}\right)$ = 5.4 grams of CH4 you must burn to emit 271 kJ of heat.

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