Question 1 In the reaction between H2O2 and I-, 15 mL of 0.30M KI, 69. mL of 0.1

Question

Question 1 In the reaction between H2O2 and I-, 15 mL of 0.30M KI, 69. mL of 0.10M H2O2 and 19 mL of 0.020M Na2S2O3 were mixed in a flask containing starch and buffer and the total volume was made up to 500mL with distilled water. The solution turned blue (indicating the presence of I2) in 1.9 minutes. Calculate the initial rate of disappearance of H2O2 in units of M min-1 to two significant figures. Hint: there are two reactions occuring here as represented by the equations 1 and 4 in the introduction of the lab manual procedure for this experiment. Question 2 For the reaction described in question 1, what is the effect on the rate of halving the concentration of Y? a. It is quartered. b. It is quadrupled. c. It is doubled. d. It is halved. e. It is the same. Question 3 For the reaction A + B --> C, the rate law is . If the initial concentration of A = 2.2 mol/L, the initial [B] = 1.4 mol/L, and the rate = 0.7 moles of product per litre per minute (M/min). Calculate the rate constant k to 2 decimal places.

Explanation / Answer

1. Rate of disappearance = change in concentration of I2/1.9 min. Using equations and mole concept find the change in concentration.................... 2. Please provide reaction rate = k(Y)^order 3. Rate law is not provided. k = rate /(a^order * b^ order)

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