2H2 O22 H2 O H -571kJ In the equation above how... - JAMB Chemistry 2005 Question
2H2 + O22 → H2+O ΔH = -571kJ
In the equation above, how much heat will be liberated if 12.0g of hydrogen is burnt in excess oxygen?
In the equation above, how much heat will be liberated if 12.0g of hydrogen is burnt in excess oxygen?
A
-1142 kJ
B
-571 kJ
C
+1142 kJ
D
-1713 kJ
correct option: d
2H2 + O22 → H2+O ΔH = -571kJ
4.0g of Hydrogen burn in air to produce -571 kJ
∴ 12.0s of Hydrogen will burn in air to produce
(12 * -571)/4 = -1713kJ
4.0g of Hydrogen burn in air to produce -571 kJ
∴ 12.0s of Hydrogen will burn in air to produce
(12 * -571)/4 = -1713kJ
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