Propane (C₂H2n+2) is burned with atmospheric air. The analysis of the products on a dry basis is as follows: CO₂ = 11% O₂ = 3.4% CO = 2.8% N₂ = 82.8% Calculate the air-fuel ratio and the percent theoretical air and determine the combustion equation.

Propane (C₂H2n+2) is burned with atmospheric air. The analysis of the products on a dry basis is as follows: CO₂ = 11% O₂ = 3.4% CO = 2.8% N₂ = 82.8% Calculate the air-fuel ratio and the percent theoretical air and determine the combustion equation.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 95QRT

See similar textbooks

Similar questions

The nitrogen content of organic compounds can be determined by the Dumas method.The compound in question is first passed over hot CuO(s): Compound N2(g) + CO2(g) + H2O(g) The gaseous products are then passed through a concentrated aqueous KOH solution to remove the CO2.The remaining gas contains N2 and water vapor.A 0.127-g sample of a compound was treated as above, producing 89.0 mL of N2 saturated with water vapor at 25 °C and 739.3 torr.What is the mass percent of nitrogen in the compound? . The vapor pressure of water at 25 °C is 23.8 torr.
Toluene, C7H8 , is burned with 30% excess air. A bad burner causes 15% of the carbon to form soot (pure C) deposited on the walls of the furnace. What is the Orsat analysis of the gases leaving the furnace
2. are the percent compositions of the flue (dry basis) if the fuel is burned stoichiometrically? Assume complete combustion. Fuel X has the following composition: C=83%, H2-7%, 0=5%, S-2%, ash=3%. What
A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas city (MCI) to Baltimore (BWI) burned 11800 lb. of Jet A fuel. Jet A fuel is kerosene based, consisting primarily of CnH2n+2 hydrocarbons, with n = 6 to 16, so the Carbon:Hydrogen ratio is close to 1:2. During this flight How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 50 miles per gallon. (Assume the density of gasoline to be 0.75kg L-1 and that carbon and hydrogen dominate the composition in a ratio 1:2. The road trip is 1082 miles.
Determine the theoretical oxygen required for the combustion of one mole of refinery gases containing 5%H2S,5%H2, 53%C3H8,2%CO2, 35%C4H10
Coal with a mass analysis of 80% carbon, 3% sulfur, 17% noncombustible ash burns completely with 120% of theoretical air. Determine the amount of SO2 produced, in kg SO2 per kg of coal.
b) Calculate the stoichiometric fuel/air mass ratio and product gas composition for the combustion of Hexane in air. (C=12, H=1, O=16, N=14)
A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas city (MCI) to Baltimore (BWI) burned 11800 lb. of Jet A fuel. Jet A fuel is kerosene based, consisting primarily of CnH2n+2 hydrocarbons, with n = 6 to 16, so the Carbon:Hydrogen ratio is close to 1:2. During this flight , how much CO2 (in kg) was released into the atmosphere? (assume the combustion of fuel was complete, so all fuel was converted into H2O and CO2).
At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropane
Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0°C and 1.00 atm. The reaction of 6.00 g of bicarbonate with excess hydrochloric acid under these conditions will produce Lof CO2. NaHCO3 + HCI CO2 + H2O + NaCI 18.2 0109 O 28.5 O 0.870 O 1.82
write the balanced chemical equation for the following: Acetylene gas is often used bby plumbers, welders, and glass blowers beacuse it burns in oxygen with an intensely blue flame. The products of the combustion of acetylene are carbon dioxide gas and water vapor. What is the coeficient in front of carbon dioxide?
Heat from Acid-Base (Neutralization) Reaction of Vinegar and Baking soda Base + Acid = Salt (general, NOT necessarily table salt) + water + maybe some other by-products Acetic acid + Sodium Bicarbonate = Water + Salt + carbon dioxide CH3COOH(aq) + NaHCO₃(s) = H2O + CH3COO-Na+ + CO2 Instructions: Measure 2 ounces of vinegar using a measuring cup and place it in the coffee-cup calorimeter. Assuming the density of vinegar is the same as water at room temperature: 1.00 g/mL, calculate the mass of the vinegar and record in Table 3. Read the thermometer and record the temperature in Table 3. Weight about 1 gram of baking soda using the weight scale. Record the exact weight of baking soda in Table 3. Put all the weight baking soda in the calorimeter and cover it with the lid right away. Observe the temperature. Swirl your calorimeter for mixing. Observe the temperature. Keep swirling until there is no change in temperature. Record the temperature in Table 3. Repeat the experiment in…