Calculate the amount of heat (in kj) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 k to 385.0 k. the specific heat capacity of ethanol is 2.42 j/g°c. calculate the amount of heat (in kj) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 k to 385.0 k. the specific heat capacity of ethanol is 2.42 j/g°c. 16.6 kj 28.4 kj 12.9 kj 73.6 kj 57.0 kj

The amount of heat required to raise the temperature of the sample from 298 to 385 Kelvin, is 16.6 kJ

Explanation:

Step 1: Given data

A 79.0 g sample of ethanol raises from 298 K to 385 K

The specific heat of ethanol is 2.42J/g°C

Step 2: Calculate the heat transfer

Q = m*Cp*ΔT

with m = the mass of the ethanol sample (in grams)

⇒ mass = 79 grams

with Cp = the specific heat capacity of ethanol (in J/g°C)

⇒ Cp = 2.42 J/g°C

with ΔT = the change of temperature (T2-T1)

⇒ ΔT = 385 K - 298K = 112 °C - 25 °C = 87

Q = 79 grams * 2.42 J/g°C * 87 = 16632.66 j = 16.6 kJ

The amount of heat required to raise the temperature of the sample from 298 to 385 Kelvin, is 16.6 kJ

is there multiple choice answers?

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