entration [I2] and rate of reaction (moles per litre per second or mol/L·s) for this reaction: H2 (g) + I2 (g) → 2 HI (g) Trial [H2] (mol/L) [I2] (mol/L) Rate  (mol/L·s) 1 0.01 0.05 0.04 2 0.02 0.05 0.08 3 0.03 0.05 0.12 4 0.05 0.01 0.02 5 0.05 0.02 0.16 6 0.05 0.03 0.54 Determine the rate law expression for this reaction.

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.

The reaction in aqueous acidic solution occurs as shown by the balanced chemical equation below: H2O2(aq) + 3 I (aq) + 2 H* (aq) 13 (aq) + 2 H20(I) In the first 40.0 seconds of the reaction, the concentration of I' changes from 1.000 M to 0.868 M. Use the information to determine the average rate of the reaction within the first 40.0 seconds of the reaction. O 3.20x103 M/s O 1.10x10-3 M/s O 4.40x10-3 M/s O 2.20x10-3 M/s

What is the average reaction rate for 2 NOB1(g) → Br,(g)+2 NO(g) over the first 10 seconds? Time [NOBr] (s) (mol/L) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 [NOBI] (mol/L) mol/L 0.0100 0.0090 0.0080 0.0070 0.0060 0.0050 0.0040 0.0030 0.0020 0.00 5.00 10.00 time (s) 6.7 x 10-3 M/s d. 3.4 x 10-4 Mls a. b. 6.7 x 10-4 Mls e. 1.3 x 10-3 M/s c. 3.3 x 10-3 M/s Oxygen gas is formed by the decomposition of potassium chlorate at high temperatures according to the reaction 2 KC10, (s) → 2 KCI(s)+3 O,(g). Suppose 1.23 g KCIO; is placed in a container connected to an open-end mercury manometer on a day when atmospheric pressure is 1.00 atm. Once the reaction is complete, the height of the mercury column in the U-tube on the side of the reaction container rises by 172 mmHg. What is the pressure of O2 gas produced by the reaction? d. 0.774 atm e. 36.7 in Hg a. 1348 torr b. 22.9 kPa c. 0.559 bar