Sulfur dioxide is oxidized to sulfur trioxide in the following sequence of reactions:2 SO2 (g) + 2 NO2 (g) ⇄ 2 SO3 (g) + 2 NO (g)2 NO (g) + O2 (g) ⇄ 2 NO2 (g)(4a): What is the overall reaction?(4b): Identify any molecule that acts as a catalyst or intermediate in this reaction

Gas Initial Concentration (M) H2 0.030 I2 0.015 HI ? Samples of three gases, H2(g) , I2(g) , and HI(g) , were combined in a rigid vessel. The initial concentrations of H2(g) and I2(g) are given in the table above. (a) The original value of the reaction quotient, Qc , for the reaction of H2(g) and I2(g) to form HI(g) (before any reactions take place and before equilibrium is established), was 5.56 . On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas.   Equilibrium was established at a certain temperature according to the following chemical equation. H2(g)+I2(g)⇄2HI(g)ΔH°rxn=−9.4kJ/molrxn;Kc=49 After equilibrium was established, the concentration of H2(g) was 0.020M . (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part ( a ). The curves must show how the concentration of each of the three gases changed…

Consider the following heterogenous reaction: 2AB(s) + C3(aq) + 4D(aq) ⇌ 2ABCD(aq) + CD2(l) The initial concentration of C3 is 0.20 M and 0.10 M for D. 5.0 g of reactant AB was also added. There were no products in the reaction flask at time 0. At equilibrium, the [D]eq = 0.03 M. (i) Will the concentration of reactant AB and product CD2 affect equilibrium? Explain why or why not. (i) Calculate the equilibrium constant, Kc for this reaction.

Predict what would happen to the amount of CO2(g) when the equilibrium is disrupted by:     Decreasing the temperature Increasing the pressure Adding more NH3(g) Adding a catalyst   DH0 > 0  therefore     (NH4)(NH2CO2)(s)  + heat  ó NH3(g)  +  CO2(g)               In A the reaction goes reverse [CO2] will decrease.      in B it goes reverse, [CO2] will decrease      in C it goes reverse [CO2] will decrease      in D, no effect

The below reaction at 927 °C has a Kc = 5.78. Calculate the concentration of NO2 at equilibrium after 299 g of NO2 and 416 g of SO2 are introduced into an empty 10.0 L container and heated to 927 °C.   NO2 (g)  +  SO2 (g)  ↔  NO (g)  +  SO3 (g

Upload the answer to this question as an image. Show your working. Consider the equilibrium step in the preparation of nitrosyl chloride, NOCI. 2NO(g) + Cl2(g) = 2NOCI(g) At a temperature of 727°C the equilibrium constant for this reaction is 3.09 × 10². The concentration of reactants and products at a particular moment in time in the realtion mixture is given below. [NO] = 0.0620 mol L1, [Cl2] = 0.538 mol L-1, [NOCI] = 0.838 mol L-1 (i) Calculate the reaction quotient, Q, at this particular time. (ii) State whether the system is at equilibrium. Justify your answer. (iii) If the system is not at equilibrium explain which way the system will move in order to reach equilibrium. Give a reason for your answer.

Apply Le Chatelier's principle and decide how (by altering temperature, pressure, and concentration) you could increase the amount of the products in the following reactions: 1)  2CO2 (g)  ----> 2CO (g) + O2 (g)     ΔH0=566 kJ 2)  2SO2 (g) + O2 (g)  ----> 2SO3 (g) Please explain and show all three alterations for each reaction.

The compound IrH;(CO)(P(C,H5);)2 exists in two forms: the meridional (“mer") and facial (“fac"). At 25°C in a nonaqueous solvent, the reaction mer → fac has a rate constant of 2.33 s', and the reaction fac → mer has a rate constant of 2.10 s-1. What is the equilibrium constant of the mer-to-fac reaction at 25°C?

8) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.075 M, [H2] = 0.051, [H2O] = 0.85, and [CH4] = 0.89, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 1 B) toward products because Q= 4.1 C) toward reactants because Q = 0.24 D) toward products because Q= 0.38 E) toward products because Q= 76 8)

Consider the following exothermic reaction: C2H4 (9) + Cl2 (g) = C2H,Cl2 (g) Part A If you were a chemist trying to maximize the amount of C2 H4C12 produced, which tactic(s) might you try? Assume that the reaction mixture reaches equilibrium. Check all that apply. decreasing the reaction volume removing C2 H¿Cl2 from the reaction mixture as it forms adding Cl2 raising the reaction temperature O O O O