Consider the reaction of hydrogen sulfide with methane, given below: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) If CH4(g) is decreasing at the rate of 0.580 mol/s, what are the rates of change of H2S(g), CS2(g), and H2(g)? H2S(g)/t =   mol/s CS2(g)/t =   mol/s H2(g)/t =   mol/s

If the rate of change of Cl2 is –0.0540M/s, what is the rate of change of NO? 2NO(g)+Cl2​(g)2NOCl(g)

10 Chlorine gas reacts with aqueous hydrogen sulfide (also known as hydrosulfuric acid) to form elemental sulfur and hydrochloric acid. Cl2(g) + H2S(aq) → S(s) + 2HCl(aq) A proposed mechanism for this reaction is Step 1 Cl2 + H2S → Cl+ + HCl + HS- Step 2 Cl + HS¯ → HCl + S (slow) (fast) Sketch a potential energy diagram for this reaction, with labels to identify activation energy, transition state, rate-determining step, and any reaction intermediate.

2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.