For the following chemical reaction: 2H2O2 → 2H2O + O2, a graph of the concentration of hydrogen peroxide (H2O2) vs time is given. Time (s) 100 150 200 250
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Consider the reaction. The graph shows the concentration of H2O2 as a function of time. a. Use the graph to calculate each quantity. (i) the average rate of the reaction between 10 and 20 s (ii) the instantaneous rate of the reaction at 30 s (iii) the instantaneous rate of formation of O2 at 50 s b. If the initial volume of the H2O2 is 1.5 L, what total amount of O2 (in moles) is formed in the first 50 s of reaction?
Hydrogen peroxide (H2O2) decomposes into water and oxygen: H2O2 (aq) -> H2O (l) + O2 (g) The data in the table below were collected for the decomposition of H2O2 at a constant temperature. If possible, determine the rate of the decomposition of H2O2 and calculate the value of the rate constant at the temperature of the experiment. Concentration of Hydrogen Peroxide as a Function of Time Time (s) [H2O2] (M) 0 100 200 0.500 0.460 0.424 500 1000 1500 0.330 0.218 0.144
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Consider the following graph and reaction. The graph above shows the concentration of H2O2 as a function of time, according to the following equation: 2 H2O2(aq) --> 2 H2O(l) + O2(g) Using the graph above, a student determined that the instantaneous rate of disappearance of H2O2 at t = 10 seconds is equal to -0.827 M/s. Given this information, what is the instantaneous rate of reaction at t = 10 s? (Do not include units in your answer. Include at least 3 sig figs in your answer).
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