100. cal of heat are added to 18.0 g of ethanol (0.581 cal/g °C) originally at 23 °C. The final temperature is .

Final temperature is 32.56 °C

Explanation:

The specific heat of a substance is the amount of heat required to raise the temperature of 1g of the substance by 1°C.

The following equation/formula is used;

Q = m × c × ΔT

Where; Q= amount of heat supplied

(cal)

M= mass of ethanol (g)

C= specific heat of ethanol

(cal/g °C)

ΔT= change in temperature (°C)

i.e. (final temperature - initial

temperature)

According to the question, Q= 100 calories (cal), M= 18g, C= 0.581 cal/g °C, initial temperature = 23°C, final temperature = ?

Hence, we insert our values into the equation;

Q = m × c × ΔT

ΔT = Q/mc

(Final T - Initial T) = Q/mc

(Final T - 23) = 100/ 18 × 0.581

(Final T - 23) = 100/10.458

Final T - 23 = 9.562

Final T = 23 + 9.562

Final T = 32.562

Hence, the final temperature of ethanol is 32.56°C

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