## Consider the reaction, C2H4(g) + H2(g) – C2H6(8), where AH = -137 kJ. How many kilojoules are released when 3.5 mol of CH4 reacts?

Question

Consider the reaction, C2H4(g) + H2(g) – C2H6(8), where AH = -137 kJ. How many kilojoules are released when 3.5 mol of CH4
reacts?
480 kJ are released
20 x 103 kJ are released
570 kJ are released
137 kJ are released​

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1 year 2021-09-05T07:44:00+00:00 1 Answers 52 views 0

1. Answer: 480 kJ of energy is released when 3.5 mol of $$C_2H_4$$ reacts.

Explanation:

The balanced chemical reaction is:

$$C_2H_4(g)+H_2(g)\rightarrow C_2H_6(g)$$  $$\Delta H=-137kJ$$

Thus it is given that the reaction is exothermic (heat energy is released) as enthalpy change for the reaction is negative.

1 mole of $$C_2H_4$$ on reacting gives = 137 kJ of energy

Thus 3.5 moles  of $$C_2H_4$$ on reacting gives = $$\frac{137}{1}\times 3.5=480 kJ$$ of energy

Thus 480 kJ of energy is released when 3.5 mol of $$C_2H_4$$ reacts.