Reaction in an ideal gas systemA2(g) + 3 B2(g) → 2 AB3(g)takes place at a temperature of 860 K in a reactor with a volume of 5.0 dm³. Atthe point, when 75% of the initial amount of substance B2 reacted, the substanceamount of this component decreases rapidly: 6.0-104 mol min-1. Determine thereaction rate at the given moment.

see attachmentExplanation:Step 1: Step 2: Step 3: Step 4:

Answered: Reaction in an ideal gas system A2(g) +…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter22: Surfaces

Section: Chapter Questions

Problem 22.44E: Are the following processes examples of homogeneous or heterogeneous catalysis? a Hydrolysis of...

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Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A +B −−→ P and the reactants are initially present in (a) their stoichiometric proportions, (b) with Bpresent initially in twice the amount.
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2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
hello, i sent this question before but the answer you rpovided for both wasnt right and i couldnt undertstand how you got the answer. can you please show me a handwritten solution for better understanding. 1a) The decomposition of ethanol at some constant temperature (above 500°C), over a copper surface, C2H5OH(g) CH3CHO(g) + H2(g) was studied by monitoring the total pressure with time.The following data were obtained: t (s) Ptotal (torr) 0 120 45 131 139 154 233 177 376 212 380 213 What will be the total pressure at t = 462 s? 1b) What is the rate constant (k)?(Include appropriate units.)
For the rate law Rate = k[A][B]3/2, the order with respect to A is __________, the order with respect to B is __________, and the overall reaction order is __________.
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The oxidation of HSO3− by O2 in an aqueous solution is a reaction of importance to the processes of acid rain formation and flue gas desulfurization. R.E. Connick et al. (Inorg. Chem. 34, 4543 (1995)) report that the reaction 2 HSO3−(aq) + O2(g) → 2 SO42−(aq) + 2 H+(aq) follows the rate law v = kr[HSO3−]2[O2]2. Given pH = 5.6 and an O2 molar concentration of 0.24 mmol dm−3 (both presumed constant), an initial HSO3− molar concentration of 50 μmol dm−3, and a rate constant of 3.6 × 106 dm9 mol−3 s−1, what is the initial rate of reaction? How long would it take for HSO3− to reach half its initial concentration?
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