Chemistry question.

[PharmLMD]

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How much heat would be generated from 10g of methane reacting with 64g of oxygen?

CH4(g) + 2O2(g) ---> 2H2O(g) deltaH = -890.3 kJ


Answer choices:

A) 5.56 kJ
B) 556 kJ
C) 1391 kJ
D) 8903 kJ

Curious as to how you solve this.

 

[Knickerbocker]

How much heat would be generated from 10g of methane reacting with 64g of oxygen?

CH4(g) + 2O2(g) ---> 2H2O(g) deltaH = -890.3 kJ


Answer choices:

A) 5.56 kJ
B) 556 kJ
C) 1391 kJ
D) 8903 kJ

Curious as to how you solve this.

For every one mole of CH4 consumed, you will generate 890.3kJ of heat. Now, you need to figure out how many moles of CH4 are actually used by determining the limiting reagent.

You have .625 moles of CH4, which could generate 1.25 moles of water. Your 2 moles of O2 could generate 2 moles of H2O. Therefore, CH4 is the limiting reagent.

You can use .625 of one mole of CH4, so multiply that by the heat/mole.