Ask Question
29 October, 05:15

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?

+5
Answers (1)
  1. 29 October, 05:38
    0
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “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 ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers