ublic concern about the increase in CO2 in the atmosphere has led to many proposals to eliminate CO2. A scientist has developed a new catalyst that makes the following reaction possible.  CO2(g) +4 H2 (g) 2 H2O(v) + CH4(g) Hydrogen would be collected from hydrolysis of water using electricity generated from solar cells. A test of the process showed on the basis of 1 mole of CO2 (entering from a different process at 800K) reacting with 4 moles H2 entering 298K, only 70% conversion of CO2 occurred. The products exit from the reactor at 1000K. Calculate the heat transfer to or from the reactor (specify which). For the Cp values from, you may use just ‘a’ and ‘b’ terms for simplicity.

A8

REACTION ENGINEERING  Consider a heterogeneous gas-phase catalytic reaction:AB(g)→A(g)+B(g) (Catalyst) The surface reaction mechanism follows three steps: AB(g) +S <----> AB*S (Adsorption)AB*S<----> B*S+A(g) (Surface reaction)B*S <---> B(g) + S (Desorption) a) Derive the initial rates (AR) of the reaction, assuming there is no product (ie., A and B) in the feed (ie., PA Pao=0), assuming adsorption is the rate determining step. Use initial pressure of AB (ie., PARA), total number of sites on the surface (C), and the rate and equilibrium constants in the expressions.Hint: Based on the reaction mechanism, only AB and B are adsorbed on the surface, i.e., there is no evidence that A alone can be adsorbed on the surface.

The equilibrium constant, Ke, for the following reaction is 1.80×10-² at 698 K. 2HI(g) H2(g) + I,(g) Calculate the equilibrium concentrations of reactant and products when 0.294 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] M [H2] M [IL] M

The reaction in which CO2 decomposes to CO and a free radical oxygen atom, O, has an activation energy of 460 kJ mol. The frequency factor is 3.6 x 10+2 s. What is the rate constant for this reaction at 312 K? (Enter your answer to two significant figures.) Rate constant = S

REACTION ENGINEERING    Consider a heterogeneous gas-phase catalytic reaction:AB(g)→A(g)+B(g) (Catalyst) The surface reaction mechanism follows three steps: AB(g) +S <----> AB*S (Adsorption)AB*S<----> B*S+A(g) (Surface reaction)B*S <---> B(g) + S (Desorption) (a) Derive the rate law assuming desorption is rate-limiting. Express the overall reaction rate (- rab) in terms of total number of sites on the surface, C. partial pressures of the gas species (ie., Pab, Pa and Pb), rate constants of adsorption, the surface reaction, and desorption (ka,ks, and kd), and the equilibrium constants of adsorption, the surface reaction, and desorption (ie., K. Ks and Kd). Hint: Based on the reaction mechanism, only AB and B are adsorbed on the surface, i.e., there is no evidence that A alone can be adsorbed on the surface.

Nitric acid is used in the starting material for the production of ammonium nitrate. The final reaction in producing ammonium nitrate is: 3HNO,(aq) – HNO,(aq) + H,O() + 2NO(9) Using your knowledge collision theory and the factors that affect the rate of a reaction, describe 3 ways that the rate of this reaction can be increased to produce more ammonium nitrate. Include specific reasons why it would increase. (A:3)

Please help me with this, I am trying to prepare for my final exam next week and I am just completely lost