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12 Dec 2019

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)

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Patrina Schowalter
Patrina SchowalterLv2
13 Dec 2019

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Related questions

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.

Propane (C3H8) is a common gas used for generating flames for cooking and camping. It undergoes a combustion reaction with excess oxygen (O2) to yeld carbon dioxide (CO2), Water (H2O) and heat. Suppose that you only have 82g propane for your trip.

A) Write the balanced stoichiometric reaction for the combustion of propane.

B) For every molecule of CO2, what is the mass percentage of C?

C) Suppose that your torch has a fixed amount of oxygen at 50g. What is the limiting reagent for your reaction and how many mols of water are produced if this reactant is consumed completely?

D) How much of the excess reagent is remaning after burning up all of the limiting reagent above?

E) Based on the chemistry described above, explain why somethering a fire puts a flame out.

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