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A 27.40 g sample of liquid mercury is initially at 158.30°C. If the sample is heated at constant pressure ( = 1 atm), kJ of energy are needed to raise the temperature of the sample to 376.20°C. How much energy in kJ is required?

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Answer:

energy required is 0.247kJ

Explanation:

The formula to use is Energy = nRdT;

Where n is number of mole

R is the molar gas constant

dT is the change in temperature

n = reacting mass of mercury / molar mass of mercury = 27.4/200.59 = 0.137

dT = final temperature - initial temperature = 376.20 - 158.30 = 217.90K

R = 8.314Jper mol per Kelvin

Energy = 0.137 x 8.314 x 217.90 = 247.12J

Energy in kJ= 247.12/1000= 0.247kJ

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