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2. How much heat is required to boil 7.3g of Ammonia? (NH 3 ) ( Δ Hvap = 23.35 kJ/mol)

1. The heat of fusion of water is 335,000 J/kg & the specific heat capacity of ice is 2,000 J/(kg C). If I introduce 2,000 J of heat to a melting block of ice with mass 1.0 kg at 0 degrees C, the final temperature is equal to: a. 0 degrees C b. 2 degrees C c. 40 degrees C d. 2,000 degrees C.

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2. How much heat is required to boil 7.3g of Ammonia? (NH 3 ) ( Δ Hvap = 23.35 kJ/mol)

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  1. 1. The heat of fusion of water is 335,000 J/kg & the specific heat capacity of ice is 2,000 J/(kg C). If I introduce 2,000 J of heat to a melting block of ice with mass 1.0 kg at 0 degrees C, the final temperature is equal to: a. 0 degrees Cb. 2 degrees Cc. 40 degrees Cd. 2,000 degrees C 2. How much heat is required to boil 7.3g of Ammonia? (NH3) (ΔHvap = 23.35 kJ/mol) 3. If 145g of water turns from gas to a liquid, how much heat is released? (the enthaply change of water of cond. is -40.7 kJ/ mol.) 4. Calculate the standard enthalpy of combustion for the following reaction: C6H12O6 (s) + 6 O2 (g) ---> 6 CO2 (g) + 6 H2O (l) To solve this problem, use the following ΔH°f values:

  2. 5. 175.0 g pure H2O was placed in a constant-pressure calorimeter and chilled to 10.0 °C. 9.80 g pure H2SO4 (also at 10.0 °C) was added, stirred and the temperature rose to 19.8 °C. • What mass increased in temperature?(b) What was Δt? • (c) Calculate the energy change for the reaction. (d) Calculate the energy change in kJ/mole of H2SO4. 6. 10.0 g of a fuel are burned under a calorimeter containing 200.0 g of H2O. The temperature of the water increases from 15.0 °C to 55.0 °C. Calculate the total heat produced (in joules) and the heat of combustion per gram of fuel.

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