Question

1. the specific heat of zinc is 0.388 j/g°c. a 700.0 g sample of zinc at 35.0°c absorbs 2.336 kj of heat. what is the final temperature of the zinc? heat = mass × specific heat × δt where δt = t_final - t_initial ☐ 26.4 °c ☐ 8.60 °c ☐ 32.1 °c ☐ 43.6 °c

Explanation:

Step1: Convert heat to joules

$2.336\ \text{kJ} = 2.336 \times 1000 = 2336\ \text{J}$

Step2: Rearrange formula for $\Delta t$

$\Delta t = \frac{\text{heat}}{\text{mass} \times \text{specific heat}}$

Step3: Calculate $\Delta t$

$\Delta t = \frac{2336\ \text{J}}{700.0\ \text{g} \times 0.388\ \text{J/g}^\circ\text{C}} = \frac{2336}{271.6} \approx 8.60^\circ\text{C}$

Step4: Solve for final temperature

$t_{\text{final}} = t_{\text{initial}} + \Delta t$
$t_{\text{final}} = 35.0^\circ\text{C} + 8.60^\circ\text{C} = 43.6^\circ\text{C}$

Answer:

$\square$ 43.6 $^\circ$C