In a particular study of the reaction described by the equation 2CH 4 O g 3 O 2

In a particular study of the reaction described by

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7.) In a particular study of the reaction described by the equation, 2CH4O(g) + 3O2(g) 2CO2(g) + 4 H2O(g), the rate of consumption of O2(g) is 0.400 mol L-1s-1. What is the rate of formation of H2O(g)? a) 1.333 mol L-1s-1b) 0.600 mol L-1s-1c) 0.333 mol L-1s-1d) 0.533 mol L-1s-1e) none rate of H2O is 4/3 that of O28.) The reaction, 2 NO(g) + O2(g) 2 NO2(g), was found to be first order in each of the two reactants and second order overall. The rate law is therefore
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2 9.) Sulfuryl chloride, SO2Cl2, is used to manufacture the antiseptic chlorophenol. The following data were collected on the decomposition of SO2Cl2at a certain temperature. SO2Cl2(g) SO2(g) + Cl2(g) Initial concentration of SO2Cl2 (M) initial rate of formation (M/s) 0.100 2.2 x 10-60.200 4.4 x 10-60.300 6.6 x 10-6What are the rate law and the value of the rate constant for this reaction? rate = k[SO2Cl2] and k = 2.2 x 10-5s-1notice as the concentration increase the so does the rate at proportion10.) For the reaction, 2 M + 2 N 2 P + Q, studies on how the initial rate of the reaction varied with concentration were carried out. Some data is given below. What is the correct rate law? Experiment [M] [N] Rate (mol L-1s-1 ) 1 0.100 0.100 0.000230 2 0.100 0.200 0.000920 3 0.200 0.200 0.000920 Rate doesn’t change when [M] changes in exp 2 and 3, thus zero order in [M]. Rate changes by a factor of 4 when the [N] doubles in exp 1 and 2 , thus [N]2, so 2ndorder in [N]. 11.) The half-life of a certain first-order reaction is 15 minutes. What fraction of the original reactant concentration will remain after 2.0 hours? 60 min1 half lifehalf lives = (2.0 hrs)= 8.0 half lives1 hr15 min
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