Question

32 mL of ethanol with an initial temperature of 11 degree C absorbs 562 J of heat. Find the final temperature of the ethanol. (Density of ethanol= 0.789 g/mL)

Answer 1

32 mL of ethanol with an initial temperature of 11 degree C absorbs 562 J of heat. Find the final temperature of the ethanol. (Density of ethanol= 0.789 g/mL)

Solution:

$$\rho = \frac {m}{V}$$

m-mass

V-volume

$\rho$-density

$$m = V * \rho$$

1) $m = 0.789 * 32 = 25.248g$

$$Q = c * m * \Delta T$$

$c$-the heat capacity of ethanol(2.46 J/gC- from source)

m-mass

Q-energy(heat)

2) $\Delta T = Q / m / c = 562 / 25.248 / 2.46 = 9.05^{\circ}C$

$$\Delta T = T _ {\text {f i n a l}} - T _ {\text {i n i t i a l}}$$

3) $T_{\text{final}} = \Delta T + T_{\text{initial}} = 11 + 9.05 = 20.05^{\circ}C$

Answer: 20.05 °C