It requires 17.10 kJ to melt 1.00 ×10^2 g of urethane [CO2(NH2) C2 H5] at 48.7^∘ C . What is the

step 1 In this problem, I can write the molar mass of urethane is given by, so M is equal to 3C plus 2O

It requires 17.10 kJ to melt 1.00 ×10^2 g of urethane...

It requires $17.10 \mathrm{kJ}$ to melt $1.00 \times 10^{2} \mathrm{g}$ of urethane $\left[\mathrm{CO}_{2}\left(\mathrm{NH}_{2}\right) \mathrm{C}_{2} \mathrm{H}_{5}\right]$ at $48.7^{\circ} \mathrm{C} .$ What is the latent heat of fusion of urethane in $\mathrm{kJ} / \mathrm{mol}$ ?

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Key Concepts

Latent Heat of Fusion

The latent heat of fusion is the energy required to convert a substance from its solid phase to its liquid phase at constant temperature. It is a crucial concept in thermodynamics and phase transitions, typically expressed per unit mass or per mole, indicating the energy needed to overcome the molecular forces maintaining the solid structure.

Molar Mass and Conversion

Molar mass is the mass of one mole of a substance, calculated by summing the atomic masses of its constituent elements. This conversion factor is essential for translating a given mass into the number of moles, enabling the comparison of energy quantities on a per-mole basis rather than per gram.

Stoichiometric Energy Calculations

Stoichiometric calculations in thermochemistry involve relating the energy change of a phase transition or reaction to the amount of substance involved. By determining the number of moles from the mass of the substance and dividing the total energy by this quantity, one can calculate properties such as the latent heat of fusion in terms of energy per mole.

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