2 H2(g) + O2(g)  2H2O(l) Time (s) [H2] [O2] [H2O]

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2 H2(g) + O2(g)  2H2O(l) Time (s) [H2] [O2] [H2O] 0.0020 0.050 0.080 0 0.0040 0.025 0.0675 0.0250 0.0060 0.018 0.064 0.032 0.0080 0.0125 0.0612 0.0375 1. What is the rate of reaction of hydrogen between 0.004 and 0.008 s? 2. Based on the coefficients of the chemical equation alone, what is the rate of oxygen reaction between 0.004 and 0.008 s? 3. What is the rate of water production during the same time period? 4. Use the concentration vs. time data to prove your answers.

Reaction [A] [B] Reaction (mol/L s) 1 0.100 0.100 1.53 x 10-4 A + B  Products Initial Rate of Reaction [A] [B] Reaction (mol/L s) 1 0.100 0.100 1.53 x 10-4 2 0.100 0.300 4.59 x 10-4 3 0.200 0.100 6.12 x 10-4 4 0.100 0.200 3.06 x 10-4 5 0.300 0.600 8.26 x 10-3 Using the above data, calculate the following: The rate law. The overall reaction order. The value of the rate constant.

C + D + E  Products Initial Rate of Reaction [C] [D] [E] Reaction (mol/L s) 1 0.400 0.300 0.560 7.14 x 10-4 2 0.100 0.500 0.200 4.55 x 10-5 3 0.100 0.200 0.200 4.55 x 10-5 4 0.400 0.300 0.750 1.28 x 10-3 5 0.100 0.300 0.560 3.57 x 10-4 Using the above data, calculate the following: The rate law. The overall reaction order. The value of the rate constant.

A + 2B + C + 4D  Products Initial Rate of Reaction [A] [B] [C] [D] Reaction (mol/L s) 1 0.25 0.30 0.60 0.15 7.20 x 10-5 2 0.75 0.30 0.60 0.15 2.17 x 10-4 3 0.25 0.30 0.20 0.15 7.20 x 10-5 4 0.75 0.30 0.60 0.45 6.51 x 10-4 5 0.75 0.44 0.60 0.15 4.67 x 10-4 Using the above data, calculate the following: The rate law. The overall reaction order. The value of the rate constant.

2MnO4- + 5ClO3- + 6H+  2Mn2+ + 5ClO4- + 3H2O Initial Rate of Reaction [MnO4-] [ClO3-] [H+ ] Reaction (mol/L s) 1 0.10 0.10 0.10 5.2 x 10-3 2 0.25 0.10 0.10 3.3 x 10-2 3 0.10 0.30 0.10 1.6 x 10-2 4 0.10 0.10 0.20 7.4 x 10-3 Using the above data, calculate the following: The rate law. The overall reaction order. The value of the rate constant