Advanced Chemistry

The combustion of 1.0 mol of sucrose liberates 5.65 x 10^3 KJ of heat. A calorimeter that has a heat capacity of 1.23 KJ/°C contains 0.60kg of water. How many grams of sucrose could be burned in the calorimeter to raise the temperature of the calorimeter and its content from 23°C to 27°C?

  1. 👍
  2. 👎
  3. 👁
  1. How many J are need to raise the T? That's
    Total Q = q(water) + q(cal)
    q(water) = mass H2O x specific heat H2O x (Tfinal-Tinitial)
    q(water) = 600 g x 4.184J/g*C x (27-23) = abut 10,000 J but that's an estimate and you should do it and all the calculations that follow much more carefully.
    q(cal) = 1,230 x dT = 1,230 x 4 = about 5,000 J
    Q = about 15,000 J = 15 kJ.
    You know 1 mol sucrose (that's 342 g sucrose) will liberate 5.65E3 kJ. So how many grams sucrose will it take? That's
    342 g sucrose x (15 kJ/5.65E3 kJ) = ? g sucrose.
    Remember all of these numbers are estimates.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    The temperature rises from 25.00 °C to 29.00 °C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ÄErxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the

  2. Chem

    The following substances undergo complete combustion in a bomb calorimeter. The calorimeter assembly has a heat capacity of 5.136 ^ C. In each case, what is the final temperature if the initial water temperature is 22.37^ C?

  3. chemistry

    A 1.000 gram sample of the rocket fuel hydrazine (N2H4) is burned in a bomb calorimeter. The temperature rises from 24.62°C to 28.16°C. The heat capacity of the calorimeter (including the water) is 5860 J/°C. Calculate the

  4. Chemistry

    The molar enthalpy of combustion of glucose is -2803 kJ. A mass of 1.000 g glucose is combusted in a bomb calorimeter. If the calorimeter contains 875 g H2O and the bomb has a heat capacity of 457 J/C, what is the temperature

  1. chemistry

    The enthalpy of combustion of benzoic acid,C6H5COOH, which is often used to calibrate calorimeters, is -3227kJ/mol. When 1.236g of benzoic acid was burned in a calorimeter, the tempurature increased by 2.345K. What is the specific

  2. Chemistry

    The heat of combustion of benzene, C6H6, is -41.74 kJ/g. Combustion of 3.65 of benzene causes a temperature rise of 4.41 C^o in a certain bomb calorimeter. What is the heat capacity of this bomb calorimeter? (kJ/C^o) So, I what I

  3. chemistry

    A 1.800 g sample of octane, C8H18, was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/°C. The temperature of the calorimeter plus contents increased from 21.12°C to 29.85°C. What is the heat of combustion

  4. Chemistry

    A quantity of 1.435g of naphthalene (C1oHs), a pungent-smelling substance used in moth repellents, was burned in a bomb calorimeter (constant volume). Consequently, the temperature of the water rose from 20.17°C to 25.84°C. If

  1. Chemistry

    Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. The heat of combustion of naphthalene is -40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a

  2. Chemistry

    Please help me figure out where I went wrong. HNO3 + KOH -> KNO3 + H2O enthalpy change = -53.4 kJ/mol 55.0 mL of 1.30 mol/L solutions of both reactants, at 21.4°C, are mixed in a calorimeter. What is the final temperature of the

  3. Chemistry

    Camphor (C10H16O) has a heat of combustion of 5903.6 kJ/mol. When a sample of camphor with a mass of 0.124 g is burned in a bomb calorimeter, the temperature increases by 2.28 oC. Calculate the heat capacity of the calorimeter.

  4. chemistry

    A 0.500 g sample of TNT (C7H5N2O6) is burned in a bomb calorimeter containing 610 grams of water at an initial temperature of 20.00ºC. The heat capacity of the calorimeter is 420 J/ºC and the heat of combustion of TNT is 3374

You can view more similar questions or ask a new question.