Given the following information: H2O(l) → H2O(g) ΔH = +44 kJWhat is the ∆H for the reaction: 2H2O(l) → 2 H2O(g)Group of answer choices+88kJ-88kJ+44kJ-44kJ
Question
Given the following information: H2O(l) → H2O(g) ΔH = +44 kJWhat is the ∆H for the reaction: 2H2O(l) → 2 H2O(g)Group of answer choices+88kJ-88kJ+44kJ-44kJ
Solution
The ∆H for the reaction: 2H2O(l) → 2 H2O(g) would be +88kJ.
Here's why:
The given reaction H2O(l) → H2O(g) has a ∆H of +44 kJ. This means that 44 kJ of energy is required to convert 1 mole of liquid water to gaseous water.
In the reaction 2H2O(l) → 2 H2O(g), we are converting 2 moles of liquid water to gaseous water.
Since the amount of energy required is directly proportional to the number of moles, we simply multiply the given ∆H by 2.
So, +44 kJ/mole * 2 moles = +88 kJ.
Therefore, the ∆H for the reaction: 2H2O(l) → 2 H2O(g) is +88kJ.
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