A hydrocarbon fuel is burnt with excess air. The Orsat analysis of the flue gas shows 10.2% CO2, 1.0% CO, 8.4% O2, and 80.4% N₂. What is the atomic ratio of H to C in the fuel?

4. Pure octane has a boiling point of 125.7 °C, but can be steam distilled with water at a tem- perature of 90 °C. Calculate the mass of octane that codistills with each gram of water and the percent composition of the vapor that is produced during the steam distillation. [Again, you'll need the vapor pressure of water at the steam distillation temp to solve this problem!] Note that if you multiply the second equation from question 3 above by the MW of both the oil and water, you get: mass oil/mass water = (P°) (MW)/ (Pwater) (MW water)

type solution in word

The composition of a gas on a dry basis is 70.0 mol% N2,70.0 mol% N2, 13.0% O2,13.0% O2, 12.0% CO2,12.0% CO2, and 5.0% CO.5.0% CO. If the mole fraction of water is 0.110,0.110, what is the gas composition on a wet basis ?

Given the Ultimate analysis of Alabama coal: Sulfur = 2.12% Hydrogen Ash = 6.40% Carbon = 77.76% Nitrogen = 2.92% Oxygen = 6.52% Moisture = 3.62% Using Ash and Moisture-free analysis, calculate the Actual A/F ratio at 15% excess air. = 4.28%

How many pound moles of air are needed to completely burn 6.5 pound moles of Benzene

Calculate the vapor phase mole fractions in equilibrium with a liquid hydrocarbon binary mix of 42% carbon tetrachloride and 58% trichloroethylene (use Antoine equation to calculate vapor pressures), for a system at 60°  Also, calculate what is the total system pressure?