Consider the following balanced equation: 4NH3 +7026 H₂O + 4NO2 [NH 3] [02] Rate (M/s) 1.0.273 0.586 0.1641 2.0.341 0.586 0.1834 3.0.405 0.779 0.1998 If the order with respect to ammonia is 1/2, what is the order with respect to oxygen? OO 0 0 0 0 0 0 O O 1/2 1 3/2 2 4 O cannot be determined

Consider the following balanced equation: 4NH3 +7026 H₂O + 4NO2 [NH 3] [02] Rate (M/s) 1.0.273 0.586 0.1641 2.0.341 0.586 0.1834 3.0.405 0.779 0.1998 If the order with respect to ammonia is 1/2, what is the order with respect to oxygen? OO 0 0 0 0 0 0 O O 1/2 1 3/2 2 4 O cannot be determined

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

Chlorine atoms in the atmosphere can react with ozone. Mathematically combine the following two reactions to create an overall balanced equation with the lowest whole-number coefficients. All chemical species in the reaction are gas-phase. Which of the following best represents the overall reaction? C1+03 → Clo+0₂ c10+ 0 → Cl + 0₂ To combine the reactions to create the overall balanced equation, you need to eliminate spectator species and only include the remaining species. O There are two lone chlorine atoms in the overall balanced reaction. O Two chlorine atoms can cause the production of two oxygen molecules. O CIO appears on the reactant and product side of the overall balanced reaction. Lone oxygen atoms are consumed by the overall reaction. O There is a net conversion of O2 to 03.
The rate of a certain reaction is given by the following rate law: =k [NO] ² [0₂] Use this information to answer the questions below. rate=] What is the reaction order in NO? What is the reaction order in O₂? What is overall reaction order? At a certain concentration of NO and O₂, the initial rate of reaction is 7.0 x 104 M/s. What would the initial rate of the reaction be if the concentration of NO were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 0.530 M/s when [NO] = 0.66 M and [0₂] = 1.5 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. k = 0 M² S M S x10 X
The rate of a certain reaction is given by the following rate law: rate = k[H,][NH;] Use this information to answer the questions below. What is the reaction order in H2? What is the reaction order in NH;? What is overall reaction order? At a certain concentration of Hz and NH3, the initial rate of reaction is 57.0 M/ s. What would the initial rate of the reaction be if the concentration of H2 were doubled? Round your answer to 3 significant digits. The rate of the reaction is measured to be 8.0 x 10* M/s when [H,] = 0.67 Mand [NH-] = 0.80 M. Calculate the value -2 k = of the rate constant. Round your answer to 2 significant digits.
The rate of a certain reaction is given by the following rate law: e=k[H₂] [NH₂] Use this information to answer the questions below. rate = What is the reaction order in H₂? What is the reaction order in NH3? What is overall reaction order? At a certain concentration of H₂ and NH3, the initial rate of reaction is 5.0 x 104 M/s. What would the initial rate of the reaction be if the concentration of H₂ were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 29.0 M / s when [H₂] = 0.99 M and [NH3] = 1.7 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. k = M 0 0 0 M 04/1 2 - 1 'S x10 X
The fate of any H2S that does get into the atmosphere is that it is ________ Reacted with nitrogen Converted rapidly to H2SO4 Cause reaction with argon gas Converted rapidly to SO2
The reaction for the Haber process, the industrial production of ammonia, is N2(g) + 3H2(g) → 2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 mol L-1 s-1. At what rate is hydrogen consumed?
According to the collision theory of kinetics, which statement best describes the rate of a chemical reaction? all collisions result in a chemical reaction. all collisions between molecules with at least a minimum kinetic energy and a catalyst result in a chemical reaction. none of the statements describes the rate of a chemical reaction. all collisions between molecules with at least a minimum kinetic energy and the proper result in a chemical reaction. orientation all collisions between molecules with at least a minimum kinetic energy result in a chemical reaction.
Br 1)what's the mechanism of the reaction? explain how does it work. fromeses Br Br 2)Give the correct stoichiometry/equivalence of the reaction (2 molecules per 1 molecule of what?) is there anything else that comes out of the reaction, if so what is it ■.
The rate of a certain reaction is given by the following rate law: rate = k[NO]²[0₂] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in O₂? What is overall reaction order? At a certain concentration of NO and O2, the initial rate of reaction is 6.0 x 105 M/s. What would the initial rate of the reaction be if the concentration of NO were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 6.0 M/s when [NO] = 1.3 M and [0₂] = 1.2 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 0 1 k = M 04/1 S -2 -1 - м - OM ²²-5-¹ S
# moles of c2h2 that will burn in the presence of 1.43 mol o2?
4
Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) → 4NO2(g) + O2 (9) At 45°C the rate constant is 6.2 x 10-4s. The reaction is first order. -1 S