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Calculate the enthalpy change in calories when 45.2 g of steam at 100$\degree$C condenses to water at the same temperature. What is the enthalpy change in joules?

Solutions

Verified$\begin{array}{c|c|c|c|c} 45.2\cancel{\text{ g H}_2\text{O}}& 1\cancel{\text{ mol H}_2\text{O}}& -40.7\cancel{\text{ kJ}}&1000\cancel{\text{ J}}&1\text{ cal}\\ \hline &18.0152\cancel{\text{ g H}_2\text{O}} & 1\cancel{\text{ mol H}_2\text{O}} &1\cancel{\text{ kJ}} & 4.184\cancel{\text{ J}} \end{array}\\\\= -2.44\times10^4\text{ cal}$

Use a series of unit conversions, including the molar heat of condensation of water and the molar mass of water, in order to determine the enthalpy change in calories.

In this problem, we need to calculate the enthalpy change in calories and joules when 45.2 g of the steam condenses at 100$^{\circ}$C to water at the same temperature.

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