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Enthalpy: Heat of reaction

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Wize University Chemistry Textbook > Thermodynamics: Part 1: (0th law, 1st law, Calorimetry, Enthalpy)

Calorimetry

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2H2(g) + O2(g) --> 2H2O(l) ΔH=-572kJ/mol


1. How much heat is produced when 72g of water gas is produced?


2. Is the reaction endothermic or exothermic?


3. We are told that O2(g) is the limiting reagent of this reaction. How many moles of O2(g) are used if the reaction releases 286kJ of heat?

More Calorimetry Questions:
Calorimetry: Heat of combustion
When 2g of rocket fuel, N2H4 is burned inside of a bomb-calorimeter, the temperature of the water rises from 22oC to 29oC. If there is 0.9kg of water and the heat capacity for the bomb is 822J/oC, what is the heat of the combustion for one mole of N2H4 in the bomb calorimeter?
Calorimetry: Heat of combustion
When 2g of rocket fuel, N2H4 is burned inside of a bomb-calorimeter, the temperature of the water rises from 22oC to 29oC. If there is 0.9kg of water and the heat capacity for the bomb is 822J/oC, what is the heat of the combustion for one mole of N2H4 in the bomb calorimeter?
Heat Capacity (bomb calorimeter)
1 gram of fried chicken is placed in a bomb calorimeter, which has a heat capacity of 10 kJ/oC. Upon combustion of the fried chicken, the temperature of the calorimeter rises by 5oC. Approximately how many nutritional calories are in 1 gram of this fried chicken if 1 nutritional calorie = 1000 calories and 1 calorie = 4.184 J ? Enter answer with 2 significant digits
Calorimetry
Equal masses of copper and iron are both heated to a temperature of 100°C. Each piece of hot metal is then placed into its own beaker containing 1 L of water. If both beakers start with the same initial temperature, which beaker of water will have the higher final temperature?
Additional information: Cu (specific heat = 0.377 J/g°C); Fe (specific heat = 0.450 J/g°C)
Calorimetry
The temperature of a 12.58 g sample of calcium carbonate (CaCO3 (s)) increases from 23.6oC to 38.2oC. If the specific heat of calcium carbonate is 0.82 J/g K, how many joules of heat are absorbed?
Calorimetry: Heat requirement
How much heat is required to convert a 15.5 g ice cube at -5.00oC to liquid water at 0oC? (The specific heat of ice is 2.09 J/g K, the specific heat of water is 4.18 J/g K, and the ΔHfus for water=334 J/g).
Calorimetry: Specific Heat Capacity
Addition of 3.10 kJ of heat is required to raise the temperature of 150 g of a liquid hydrocarbon from 23.0oC to 44.0oC. What is the specific heat capacity of this hydrocarbon?
A bomb calorimeter assembly has a heat capacity of 650 J/°C. Inside the bomb calorimeter 2.5g of a fuel compound is burned in excess oxygen and the temperature of the bomb calorimeter increases by 48 °C. What is the value for qrxn amount of heat released per gram of compound burned?
Please report your answer to three significant figures in kJ/g. Do NOT include units in the answer field
Water can absorb infrared radiation at a wavelength of1.06×104 m{\small 1.06\times10^4 \text{ m}}. If a 180 g sample of water is irradiated at this wavelength, calculate the number of photons required to raise the temperature by 25.0°C(CH2O=4.184Jg°C){\small \degree \text{C} \left(C_{H_2O} =4.184\frac{J}{g\degree C} \right)}
Calorimetry: Heat of combustion
When 2g of rocket fuel, N2H4 is burned inside of a bomb-calorimeter, the temperature of the water rises from 22oC to 29oC. If there is 0.9kg of water and the heat capacity for the bomb is 822J/oC, what is the heat of the combustion for one mole of N2H4 in the bomb calorimeter?
When 1.00 kg of lead (specific heat = 0.13 J / g °C) at 125 °C is added to a quantity of water at 18.0 °C, the final temperature of the lead-water mixture is 32.0 °C. What is the volume of water present? Note: the density of H2O(l) is 1.00 g/mL and the specific heat capacity is 4.18 J / g oC.
Calorimetry: Specific Heat
A piece of metal weighing 58g was heated to 100oC and then added to 100mL of water. The water's temperature was initially 22oC and after the metal was added the temperature was 26oC. What is the specific heat of the metal?