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Question

The combustion of hydrogen-oxygen mixture is used to produce very high temperatures (=2500 C) needed for certain types of welding operations.
H2(g)+12O2(g)H2O(g); ΔH=230.9 kJ
Quantity of heat, (in kJ) evolved when a 200 g mixture containing equal parts of H2 and O2 mass is burned, is

A
2.72×103 kJ
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B
1.36×103 kJ
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C
1.44×103 kJ
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D
4.3524×104 kJ
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Solution

The correct option is C 1.44×103 kJ
Total mass =200 g
O2 taken =100 g=10032=3.125 mol
H2 taken =100 g=1002=50 mol
O2 is the limiting reagent
H2 used in combustion =6.25 mol
Thus, heat evolved =230.9 kJ mol1×6.25 mol
=1443.125 kJ=1.44×103 kJ

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