Question

1. You have the following data for the following reaction at a particular temperature: H2PO. Mag) + OH(aq) — HPO.2"(aq) + H20(1) Experiment (OH). (mol/L) [H2PO4) (mol/L) 0.0030 Initial Rate(mol/L min) 0.00040 0.0020 0.0030 0.00120 0.0180 0.0090 0.00040 0.0060 Write the rate law expression for this reaction and the value of the rate constant (with its appropriate units). 2. You have run a reaction by mixing 4.00 mL of 4.0 Macetone, 4.00 mL of 1.0 M HCI, 2.00 mL of 0.0050 M 13, and 4.00 mL of water and measuring the time for the color of Iz to disappear. If it takes 300.0 seconds for the color to disappear, calculate the rate of the reaction. Hint: Read the Lab Manual!.

Answer 1

Answer (1 Rate law: Rate = K[H₂ Pog] * [OH-] where, kis rate constant x and y are order of reaction with respect to H₂POg and oth respectively. Run 1: 0.0020 = kx (0.0030) *x (0.00040) - Runa: 0.0180 = K*(0.0030) *x (0.00120) - ) Run 3 : 0.0060 = kx (0.0090)** (0.00040) - ) equation - (1) & equation - (2) : 10.000 40 jy _ 0.0020 0.0180 0.00120 a, y = 2 equation - (d = equation - (3) : 10.0030 ) 0.0090 / 0-0020 0.0060 or x rate law: = 1 Kate= K [H2POą] [OH-] / sog Rate K = [H2POT [OH-72 (mol/L) (minst = 4.2 X10 0.0020 _ Run 1 : 42x 10° (0.0030x (0.00040)2 = 0.0180 Runa: 0.0030)*(0.0012012- 0.0060 Run 3o (0.0090XC6-00040)2 .: Average K= (4.2x106) + (1.28100) + (4.2x106) 42 X10 lor min 3 - 4-2 X10% (mu?) ? min