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One (1) mol of Propane is placed in an adiabatic, constant pressure combustion chamber at 25 C. The reaction will follow: C3H8 + 5O2 → 3CO2 + 4H2O What is the final temperature of the system under those various cases? Assume complete combustion

a.. it is mixed with a stoichiometric amount of oxygen and reacts to form H2O and CO2

b. It is mixed with a stoichiometric amount of air (same reaction than a)

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Related questions

1) What is the final temperature when heat of 1100kJ is added to 30moles of SO2 initially at 300 Celsius in
a steady flow heat exchanger at atmospheric pressure

2)One (1) mol of Propane is placed in an adiabatic, constant pressure combustion chamber at 25 C.
The reaction will follow: C3H8 + 5O2 → 3CO2 + 4H2O
What is the final temperature of the system under those various cases? Assume complete
combustion.
a. it is mixed with a stoichiometric amount of oxygen and reacts to form H2O and CO2

b. It is mixed with a stoichiometric amount of air (same reaction than a)

One mole of propane, C3H8 is placed in an adiabatic (isolated),constant pressure combustion chamber at 25C and allowed to reactwith a stoichiometric amount of oxygen and reacts to form H2O andCO2

1 C3H8 + 5 O2 -----> 4 H2O (g) + 3 CO2 (g)

Delta H C3H8 = -103.85 kJ/mole, Delta H CO2= -393.51 kJ/mole,Delta H H2O= -241.82 kJ/mole.

What is the enthalpy change for thereaction?

A 16.0 gram sample of propane gas (C3H8) is burned according to the equation C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g).

In an enclosed container with a volume of 2.25L at a temperature of 322K.

If the sample of propane burns completely and no oxygen remains in the container, calculate the mole fractions of CO2 and H2O.

Calculate the total pressure in the container after the reaction.

Calculate the partial pressure of CO2 and H2O in the container after the reaction.

If 12.1 grams of propane is burned in the presence of 10.2 atm of oxygen at the above temperature and volume conditions, determine the theoretical yield of H2O.

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