In a closed combustion vessel, propane (C3H8) and air are mixed at equivalence ratio of 1.11,...

In a closed combustion vessel, propane (C3H8) and air are mixed at equivalence ratio of 1.11, temperature of 298 K, and pressure of 1 bar. The mixture is burned to produce solely CO2, CO, H2O, and N2. The heat rejected from the vessel is 820 MJ/kmol of fuel. What are the final temperature and final pressure of the mixture? Since neither O2 nor H2 is present in the burned gas, dissociation can be neglected.

Expert Solution

samet mamat answered 2 years ago

Calculate the mole fraction when a sample of propane (C3H8) is placed in a closed vessel...

Calculate the mole fraction when a sample of propane (C3H8) is placed in a closed vessel together with an amount of O2 that is 2.15 times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Assume all chemical species are in the gaseous phase.

Calculate the theoretical A/F ratio for the complete combustion of propane (C3H8) on mole basis and...

Calculate the theoretical A/F ratio for the complete combustion of propane (C3H8) on mole basis and mass basis. Also, calculate the equivalence ratio for the following reaction: C3H8 + 7O2 + 26.32N2 → 3CO2 + 4H2O + 2O2 + 26.32N2

In a furnace, 76 lbs propane C3H8 are burned with 17.2% excess air for complete combustion....

In a furnace, 76 lbs propane C3H8 are burned with 17.2% excess air for complete combustion. What is the percent CO2 in combustion products? Round your answer to the one decimal place.

Why the temperature increase when flow rate of air increase in air-ch4 combustion, and equivalence ratio...

Why the temperature increase when flow rate of air increase in air-ch4 combustion, and equivalence ratio always uniforms ??

(a) Let us consider CH4 combustion in air with an equivalence ratio of 0.9, where we...

(a) Let us consider CH4 combustion in air with an equivalence ratio of 0.9, where we have air flow rate of 400 kg/s. (1) calculate the required flow rate of CH4 (in kg/s), the air-to-fuel ratio on mole basis, and the mole and mass fractions of CO2, H2O, O2, N2 in the product stream. (2) If reactants enter the combustion chamber at 790K, and the products are found to leave the chamber at 1900K, calculate the net heat loss from...

Propane is mixed with 20% excess air (propane air mixture is initially at 25 °C and...

Propane is mixed with 20% excess air (propane air mixture is initially at 25 °C and 2.0 atm) and combusted at atmospheric pressure. It is assumed that the heat transfer between the chamber and the surroundings is negligible. In addition, you may assume that heat capacities of the gases are constant and that the reaction proceeds to 100% conversion. (30 points) a) Determine the flame temperature of the burner. b) Determine the flame temperature if 25% of the heat generated...

In a combustion device, a mixture of 82 lbs of butane and 212 lbs propane C3H8...

In a combustion device, a mixture of 82 lbs of butane and 212 lbs propane C3H8 are burned with just enough air for complete combustion. How many lbs of total combustion products are formed? Round your answer to the nearest whole number

A sample of propane gas (C3H8) having volume of 1.80L at 25oC and 1.65atm was mixed...

A sample of propane gas (C3H8) having volume of 1.80L at 25oC and 1.65atm was mixed with a sample of oxygen gas having a volume of 35.0L at 31oC and 1.25atm. The mixture was ignited to form carbon dioxide and water. Write the balanced reaction. What is the limiting reagent? What is the maximum number of grams of water which can form from this reaction? Find the number of moles of excess reactant at STP.

The combustion reaction of propane is as follows. C3H8(g) + 5 O2(g) → 3 CO2(g) +...

The combustion reaction of propane is as follows. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. Answer in KJ/mol reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 3 C(s) + 4 H2(g) → C3H8(g) ΔH = −103.8 kJ/mol

At 25°C, the standard enthalpy of combustion of gaseous propane (C3H8) is –2219.0 kJ per mole...

At 25°C, the standard enthalpy of combustion of gaseous propane (C3H8) is –2219.0 kJ per mole of propane, and the standard enthalpy of combustion of gaseous propylene (C3H6) is –2058.3 kJ per mole of propylene. What is the standard enthalpy change for the following reaction at 25°C? C3H6(g) + H2(g) → C3H8(g) Substance ∆H°f (kJ/mol) CO2(g) –393.5 H2O(l) –285.8 a) +160.7 kJ b) –160.7 kJ c) +104.7 kJ d) –20.4 kJ e) –125.1 kJ

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