A can with water is heated up due to a chemical reaction: $\mathrm{CaO}+\mathrm{H} 2 \mathrm{O}-\mathrm{Ca}(\mathrm{OH}) 2$ Calculate the mass of water that is needed to heat up $400 \mathrm{~mL} \mathrm{H} 2 \mathrm{O}$ about $75 \mathrm{~K}$.

Enthalpy of formation CaO: $\Delta \mathrm{H}(\mathrm{CaO})=-635,09 \mathrm{~kJ} / \mathrm{mol}$. Enthalpy of formation $\mathrm{Ca}($ $\mathrm{OH}) 2: \Delta \mathrm{H}(\mathrm{Ca}(\mathrm{OH}) 2)=-986,1 \mathrm{~kJ} / \mathrm{mol}$. Enthalpy of formation $\mathrm{H} 2 \mathrm{O}: \Delta \mathrm{H}(\mathrm{H} 2 \mathrm{O}$ )$=-285,83 \mathrm{~kJ} / \mathrm{mol}$

Heat capacities: $\mathrm{c}(\mathrm{H} 2 \mathrm{O})=4,18 \mathrm{~J} /\left(\mathrm{g}^{*} \mathrm{~K}\right) . \mathrm{c}($ can + reaction substances $): 449 \mathrm{~J} / \mathrm{K}$

Question

A can with water is heated up due to a chemical reaction: $\mathrm{CaO}+\mathrm{H} 2 \mathrm{O}->\mathrm{Ca}(\mathrm{OH}) 2$ Calculate the mass of water that is needed to heat up $400 \mathrm{~mL} \mathrm{H} 2 \mathrm{O}$ about $75 \mathrm{~K}$.

Enthalpy of formation CaO: $\Delta \mathrm{H}(\mathrm{CaO})=-635,09 \mathrm{~kJ} / \mathrm{mol}$. Enthalpy of formation $\mathrm{Ca}($ $\mathrm{OH}) 2: \Delta \mathrm{H}(\mathrm{Ca}(\mathrm{OH}) 2)=-986,1 \mathrm{~kJ} / \mathrm{mol}$. Enthalpy of formation $\mathrm{H} 2 \mathrm{O}: \Delta \mathrm{H}(\mathrm{H} 2 \mathrm{O}$ )$=-285,83 \mathrm{~kJ} / \mathrm{mol}$

Heat capacities: $\mathrm{c}(\mathrm{H} 2 \mathrm{O})=4,18 \mathrm{~J} /\left(\mathrm{g}^{*} \mathrm{~K}\right) . \mathrm{c}($ can + reaction substances $): 449 \mathrm{~J} / \mathrm{K}$

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Calculate the total heat required to raise the temperature of water**: To find the total heat required to raise the temperature of 400 mL of water by 75 K, we use the formula $q = mc\Delta T$, where $m$ is the mass of the water, $c$ is the specific heat capacity of water, and $\Delta T$ is the change in temperature. ‖ ‖ 2 ⋮ **Convert volume of water to mass**: Assuming the density of water is approximately $1 ext{ g/mL}$, the mass of 400 mL of water is 400 g. ‖ ‖ 3 ⋮ **Calculate the heat required for the water**: Using the specific heat capacity of water ($4.18 ext{ J/g}\cdot ext{K}$), the heat required is $q = (400 ext{ g}) imes (4.18 ext{ J/g}\cdot ext{K}) imes (75 ext{ K})$. ‖ ‖ 4 ⋮ **Calculate the enthalpy change for the reaction**: The enthalpy change for the reaction can be found using the enthalpies of formation: $\Delta H_{ ext{reaction}} = \Delta H_{ ext{products}} - \Delta H_{ ext{reactants}}$. ‖ ‖ 5 ⋮ **Determine the mass of water needed for the reaction**: The mass of water needed can be found by equating the heat absorbed by the water to the enthalpy change of the reaction. ‖ ∻Answer∻ ⚹ [Insert final answer here] ⚹ ∻Key Concept∻ ⚹ Thermochemistry and heat transfer ⚹ ∻Explanation∻ ⚹ The problem involves calculating the heat required to raise the temperature of water and then relating it to the enthalpy change of a chemical reaction to find the mass of water needed. ⚹◊What is the total heat released in the reaction between calcium oxide and water⍭ Generate me a similar question◊

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