From the data below, calculate the total heat (in J) needed to convert 25.00 g of ice at -7.25 °C to liquid water at 0.45 °C: m.p. at 1 atm: 0.0 °C ΔH fus: 6.02 kJ/mol c liquid: 4.184 J/g*°C c solid: 2.09 J/g*°C
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Adi S.
From the data below, calculate the total heat (in J) needed to convert 30.00 g of ice at -2.75°C to liquid water at 0.250°C: m.p. at 1 atm: 0.0°C ΔH fus: 6.02 kJ/mol c liquid: 4.184 J/g·°C c solid: 2.09 J/g·°C
From the data below, calculate the total heat (in $\mathrm{J}$ needed to convert 22.00 g of ice at $-6.00^{\circ} \mathrm{C}$ to liquid water at $0.500^{\circ} \mathrm{C} :$ $\mathrm{mp}$ at 1 atm: $0.0^{\circ} \mathrm{C}$ $\Delta H_{\mathrm{fus}}^{\circ} : \quad 6.02 \mathrm{kJ} / \mathrm{mol}$ $c_{\text { liquid }} : \qquad 4.21 \mathrm{J} / \mathrm{g} \cdot^{\circ} \mathrm{C} \quad c_{\mathrm{solid}} : 2.09 \mathrm{J} / \mathrm{g} \cdot^{\circ} \mathrm{C}$
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