How much faster will a reaction be at 40 °C than at 25 °C, when its activation energy (Ea) is equal to 18.0 kcal mol–1? [R = 1.986 × 10-3 kcal mol–1 K–1; °K = °C + 273.15]

Consider the following reaction: 2H₂S(g) + SO₂(g) — 3S(s) + 2H₂O(g) A reaction mixture initially containing 0.520 M H₂S and 0.520 M SO₂ was found to contain 1.2×10-³ M H₂O at a certain temperature. A second reaction mixture at the same temperature initially contains [H₂S] = 0.255 M and [SO₂] = 0.315 M. Part A Calculate the equilibrium concentration of H₂O in the second mixture at this temperature. Express your answer using two significant figures. IVE ΑΣΦ [H₂O] = Submit Request Answer ? M

⦁    4.  Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.

For the reversible reaction: N 2 (g)+ O 2 (g) = 2 NO (g) AH= 181 kJ (a) What will happen to the concentrations of NO at equilibrium if O, is added? (b) What will happen to the concentrations of NO at equilibrium if NO is removed? (c) What will happen to the concentrations of NO at equilibrium if the volume of the reaction vessel is increased? (d) What will happen to the concentrations of NO at equilibrium if the temperature of the system is decreased? (e) What will happen to the concentrations of N,, 0,, and NO at equilibrium if a catalyst is added?

The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K. A sample of gas in which [H2S] = 5.96 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.

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.

For the endothermic reaction  A (aq) + B (aq) → C(aq) + D(s) What direction does the reaction proceed when some B is removed?                          Does the increase in temperature increase, decrease, or not affect the concentration of C?                                   Does the addition of more D increase, decrease, or not affect the concentration of C?                                   Does the addition of water to a reaction vessel where equilibrium of this reaction has been established increase, decrease, or not affect the concentration of C?

Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.

H- HHH H │ │ | I H -H+2H-H The above reactants would undergo a (n) catalyst reaction

The steam reforming reaction of methane follows this chemical equation: CHA(g) + H50(g) - CO(g) + 3 H2(g) A H° = +193 kJ/mol At 298 K the reaction lies far to the reactant side with a very small equilibrium constant of 2.35 × 10-23. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100 K?