ΔH for the following reaction is -180 kJ. How much heat is released when 10 moles of Na are allowed to react? 2 Na(s) + 2 H2O(l) –> 2 NaOH(aq)+ H2(g) Group of answer choices900 kJ1000 kJ800 kJ700 kJ
Question
ΔH for the following reaction is -180 kJ. How much heat is released when 10 moles of Na are allowed to react? 2 Na(s) + 2 H2O(l) –> 2 NaOH(aq)+ H2(g) Group of answer choices900 kJ1000 kJ800 kJ700 kJ
Solution
The given reaction is:
2 Na(s) + 2 H2O(l) –> 2 NaOH(aq) + H2(g)
The ΔH for this reaction is -180 kJ. This means that 180 kJ of heat is released when 2 moles of Na react with 2 moles of H2O to form 2 moles of NaOH and 1 mole of H2.
We are asked to find out how much heat is released when 10 moles of Na react.
First, we need to find out how much heat is released per mole of Na. Since the reaction releases 180 kJ of heat for 2 moles of Na, the heat released per mole of Na is 180 kJ / 2 = 90 kJ.
Therefore, when 10 moles of Na react, the heat released is 10 moles * 90 kJ/mole = 900 kJ.
So, the answer is 900 kJ.
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