The reduction of NO to N, with H,;2NO(g) + 2H2(g) = N2(g) + 2H,0(g), is found to have the following experimentally determined rateequation: Rate =k[NO]²[H,]If the concentration of NO and H, were doubled then the rate of the reaction would:Decrease four foldIncrease four foldIncrease two foldIncrease eight fold

Given: Chemical Equation 2 NO (g) + 2 H 2 (g) → N 2 (g) + 2 H 2O (l) Rate = k[NO]2[H2]

The reduction of NO to N, with H: 2NO(g) + 2H2(g) = N2(g) + 2H,0(g), is found to have the followving experimentally determined rate equation: Rate = k[NO] [H;] If the concentration of NO and H, were doubled then the rate of the reaction would: Decrease four fold Increase four fold O Increase two fold Increase eight fold

The reduction of NO to N, with H: 2NO(g) + 2H2(g) = N2(g) + 2H,0(g), is found to have the followving experimentally determined rate equation: Rate = k[NO] [H;] If the concentration of NO and H, were doubled then the rate of the reaction would: Decrease four fold Increase four fold O Increase two fold Increase eight fold

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

???
:::;;;;(((( Question and it’s parts
Here we compare the first order and second order reaction based on Integrative rate laws. Reaction 1: A first order reaction (A à products) has the rate constant k = 0.483 min-1 (Rate = k[A]), and the initial concentration of reactant A is 0.800 M. Reaction 2: A second order reaction (B à products) has the rate constant k = 0.483 M-1 min-1 (Rate = k[B]2), and the initial concentration of reactant B is 0.800 M. Which of the following statements is true about these two reactions? Choose one option only Options: a. Reaction 1 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 2 will. b. Reaction 2 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 1 will. c. Reaction 1 and Reaction 2 will take the same amount of time to change the reactant concentration from 0.800 M to 0.400 M. d. None of the above
Consider this reaction: 2N,0, (e) - 2N,0, te +0,e) At a certain temperature it obeys this rate law. rate - (8.45 M[N,0, %3D Suppose a vessel contains N,O, at a concentration of 0.460M. Calculate how kong it takes for the concentration of N,O, to deorease to 0.0874M. You may assume no other reaction is important Round your answer to 2 significant digits.
The decomposition of N₂O, can be described by the equation 2N₂O5(soln) -> - →→→ 4NO₂ (soln) + O₂(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. t (s) 0 225 556 755 average rate of reaction: PRE average rate of reaction: [N₂O,] (M) Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 225 s? average rate of reaction: 2.381 2.067 What is the average rate of reaction for the time interval from 225 s to 556 s? TOOLS 1.678 1.481 What is the average rate of reaction for the time interval from 556 s to 755 s? a M/s M/S M/s Rese Question Sou 994
3. Sucrose decomposes in aqueous solution into a mixture of two sugars, glucose and fructose. C„H„0, (aq) + H,0(1) I C,H,,0,(aq) + C,H,„O,(aq) The observed initial rates of decomposition of sucrose at two different initial sucrose concentrations at 25°C are: Rate ( M sec ') [Sucrose] 0.1 8.5 X 10 -3 1.71 X 102 0.2 Find the dependence of the reaction rate on the concentration of sucrose and compute the rate constant for the reaction.
See image below.
The decomposition of N2O5 can be described by the equation 2N2O5(soln)⟶4NO2(soln)+O2(g) Consider the data in the table for the reaction at 45 ∘C in carbon tetrachloride solution. ? (?) [N2O5] (?) 0 1.967 145 1.796 446 1.486 735 1.239 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 145 s? What is the average rate of reaction for the time interval from 145 s to 446 s? What is the average rate of reaction for the time interval from 446 s to 735 s?
:/::(::(::
??
help w this question plz
3. What is the rate of reaction with respect to HI(g) in the following reaction: H₂(g) + I2(g) → 2HI(g) (a) 22[Hr] dt 1 d[HI] (b) - 2 dt 1 d[HI] 2 dt (d) -2 [HI] dt (c)