Propane gas (C3H6 (g)) is withdrawn from a 100.0 L cylinder at 25.0 oC and is burned at constant pressure in an excess of oxygen. The pressure in the cylinder falls from 2.25 atm to 1.05 atm.  The liberated heat is then used to raise the temperature of 65.5 L of water from 25.0 oC to 56.7 oC. What % of the heat of combustion was absorbed by the water (d = 1.00 g/mL)?   Specific heat capacity of water = 4.18 J/g/oC Δ Hfo(H2O(l)) = -285.8 kJ/mol,    Δ Hfo(O2(g)) = 0 kJ/mol,    Δ Hfo(CO2 (g)) = -393.5 kJ/mol   Δ Hfo(C3H6 ) = -103.8 kJ/mol

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6334 g sample of acetylsalicylic acid (C9H8O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.100×103 g of water. During the combustion the temperature increases from 22.68 to 25.23 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 929.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of acetylsalicylic acid based on these data. C9H8O4(s) + 9O2(g) 4 H2O(l) + 9 CO2(g) + EnergyMolar Heat of Combustion =   how many kJ/mol

Consider the following chemical reaction: C2H6O(l) + O2(g) -----------> CO2(g) + H2O(g)  0.8100 g C2H6O(l) is burned in bomb calorimeter.   The initial temperature is 22.000 oC and the temperature rises to 28.200 oC.     Calculate the heat of reaction at constant pressure  at 22.0 oC in kJ/mole C2H6O      The heat capacity of calorimeter is 10.50 kJ/ oC. C= 12.01 g/mole, H = 1.008 g/mole,  O = 16.00 g/mole

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat is liberated or absorbed by the reaction that produces 355 mL of nitrogen gas at 25°C and 737 mm Hg?

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol

Hw.77.

Constant is 4.184