Question

In a phase change of water between the liquid and the gas phases, 770.1 kj of energy was released by the system. What was the product, and how much of it was formed in the phase change? (data: h2o(l) h2o(g) h = 44.01 kj/mol.)

Answer 1

17.5 moles liquid water was produced.

Step by step explanation:

The given chemical reaction is as follows.

$\bold{H_{2}O(l)\rightarrow H_{2}O(g)}$

The $\Delta H=44.01\,kJ/mol$

The given value is positive and it indicates the endothermic reaction.

770 kJ of energy released during the conversion of liquid state to gaseous state.

one mole of water conversion required 44 kJ/moll of energy.

For 770 kJ energy---------------------?

$\bold{=\frac{1}{44}\times 770kJ=17.5\,moles}$

Therefore, 17.5 moles liquid water was produced.

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