Calculate the value of the equilibrium constant and the equilibrium composition of the product gas at 1000 K for the following homogenous gas-phase reaction: C3H8 + 3 H2O ↔ 3 CO + 7 H2 Steam is fed to the reactor in a 1-to-8 ratio and the reactor is operating at atmospheric pressure.

Into a combustion reactor, hexane at 55 mol and 25% excess dry air are fed. The fractional conversion of hexane is 85%. Assume that air is 21 mol% oxygen and 79 mol% nitrogen. The governing equation for the combustion reaction is: 2 C6H14 + 19 O2 → 12 CO2 + 14 H2O a. Draw a complete flowchart of the process. Clearly state any assumptions. b. Perform a degree-of-freedom analysis (atomic species DOF). c. What is the mole fraction of carbon dioxide in the flue gas on a dry basis? PLEASE Solve using ATOMIC SPECIES, thank you

QUESTION 9 Regarding the following reaction at constant temperature, calculate the ratio of Kx at total pressure of 5.0 bar to that at 1.5 bar. Please enter your answer with 1 decimal. For example, 0.567 is written as 0.6. H₂CO (g) = CO (g) + H₂ (g).

Q1: For elementary reaction A +B the equilibrium conversion is 0.8 at 127°C and 0.5 at 227°C. What is the heat of reaction?