(Solved): The specific heat capacities of gold and copper are \( 0.129 \mathrm{~J} / \mathrm{g} \cdot{ }^{\ci ...

The specific heat capacities of gold and copper are \( 0.129 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} \) and \( 0.387 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} \), respectively. At \( 25^{\circ} \mathrm{C}, 230 \) joules of heat is added to \( 10.0 \mathrm{~g} \) samples of pure gold and copper. Select the correct statement about temperature changes. (Notes You can answer this question without detalled calculations.) a) Both samples will eqerience the same increase in temperature. b) The temperature of the gold sample will rise higher than that of the copper sample. c) The temperature of the copper sample will rise higher than that of the gold sample. d) Both samples will experience the same decrease in temperature. Question 7 (1 point) How much heat will be required to convert one mole of ice at \( -5^{\circ} \mathrm{C} \) to steam at \( 105^{\circ} \mathrm{C} \) ? \( \begin{array}{ll}\Delta H_{\text {fus }} & 6010 \mathrm{~J} / \mathrm{mol} \\ \Delta H_{\text {vap }} & 40,670 \mathrm{~J} / \mathrm{mol} \\ C_{p} \text { (ice) } & 37.1 \mathrm{~J} /\left(\mathrm{mol} \cdot \mathrm{H}^{\circ \mathrm{C}}\right. \\ C_{p} \text { (water) } & 75.3 \mathrm{~J} /\left(\mathrm{mol} \cdot{ }^{\circ \mathrm{C}}\right)\end{array} \) \( C_{p} \) (steam) \( 33.6 \) Jimonteci a) \( 37.1 \mathrm{ka} / \mathrm{mol} \) b) \( 40.7 \mathrm{~kJ} / \mathrm{mol} \) c) \( 46.0 \mathrm{kd} / \mathrm{mol} \) d) \( 54.6 \mathrm{~kJ} / \mathrm{mol} \) e) \( 75.3 \mathrm{~kJ} / \mathrm{mol} \)