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ΔH for the following reaction is -180 kJ. How much heat is released when 100 g of Na are allowed to react? The molar mass of sodium is 23.0 g/mol. 2 Na(s) + 2 H2O(l) –> 2 NaOH(aq) + H2(g) Group of answer choices491 kJ691 kJ591 kJ391 kJ

Question

ΔH for the following reaction is -180 kJ. How much heat is released when 100 g of Na are allowed to react? The molar mass of sodium is 23.0 g/mol. 2 Na(s) + 2 H2O(l) –> 2 NaOH(aq) + H2(g) Group of answer choices491 kJ691 kJ591 kJ391 kJ

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Solution

To solve this problem, we need to follow these steps:

  1. First, we need to determine the number of moles of Na in 100 g. We can do this by dividing the mass of Na by its molar mass. So, 100 g ÷ 23.0 g/mol = 4.35 mol.

  2. The given reaction shows that 2 moles of Na react to release -180 kJ of heat. Therefore, 1 mole of Na would release -180 kJ ÷ 2 = -90 kJ of heat.

  3. Now, we can calculate the amount of heat released by 4.35 moles of Na. This is done by multiplying the number of moles by the heat released per mole. So, 4.35 mol x -90 kJ/mol = -391.5 kJ.

  4. Since the heat is released, it is exothermic, and the sign is negative. However, in terms of magnitude, 391.5 kJ of heat is released.

So, the answer is 391 kJ.

This problem has been solved

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