Nitrogen dioxide reacts with carbon monoxide by the overall equation NO:(9) + CO(g) → NO(9) + CO2 (9) At a particular temperature, the reaction is second order in NO, and zero order in CO. The rate constant is 0.515 L/(mol - s). How much heat energy evolves per second initially from 7.25 Lof reaction mixture containing 2.40 x 102 M NO,? NO: (9) + NO(g) + co(g) -110.5 kJ/mol + CO2(9) -393.5 kJ/mol AH; = 33.10 kl/mol. 90.29 kJ/mol Assume the enthalpy change is constant with temperature. Energy = kJ/s

Nitrogen dioxide reacts with carbon monoxide by the overall equation NO:(9) + CO(g) → NO(9) + CO2 (9) At a particular temperature, the reaction is second order in NO, and zero order in CO. The rate constant is 0.515 L/(mol - s). How much heat energy evolves per second initially from 7.25 Lof reaction mixture containing 2.40 x 102 M NO,? NO: (9) + NO(g) + co(g) -110.5 kJ/mol + CO2(9) -393.5 kJ/mol AH; = 33.10 kl/mol. 90.29 kJ/mol Assume the enthalpy change is constant with temperature. Energy = kJ/s

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

None
At A reaction of A products follow a second constant of 3.76 X65M's, order → Kinetics with a
Delta G0 for a reaction can only be converted into Keq or E0cell when the Kinetics of the process is fast. Is this a true statement?
The reaction below is a decomposition reaction of HI. 2HI → H₂ + 1₂ In this reaction, the following data were generated. T (°C) 508 427 393 K (cm3/mol.s) 1.059x10-¹ 3.1x10-³ 5.88x10-4 Find the complete rate equation for this reaction [i.e. r = ƒ(T)ƒ(C)]. 356 8.09x10-5 283 9.42x10-7
Chlorine monoxide (ClO) accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, ClO decomposes according to the equation: 2C1O (g) → Cl2 (g) + O2 (g) The kinetics of this reaction were studied in a laboratory experiment at 298K, and the data are shown in the table below. (a) Determine the order of the reaction (b) Determine the rate law expression (c) Determine the value of the rate constant, k, at 298K. Time (ms) [CiO] (M) In [ClO] cioj (M-1) [CiO] 6.67 × 107 1.39 x 108 -8- 1.50 x 10 7.19 x 10 4.74 × 10 -18.0 6- 10 -18.8 6- 20 -19.2 2.11 x 108 6- 30 3.52 х 10° -19.5 2.84 x 108 6- 40 2.81 x 10 -19.7 3.56 x 108 6- 100 1.27 x 10 -20.5 7.87 x 108 10 200 6.60 x 10- -21.1 1.52 x 10°
In the reaction N2 +3 H2 à 2NH3 if the Δ[H2]/t is -1.5 x 10-3 M/s, What is the Δ[NH3] at the same point? (How fast is the NH3 being produced)?
A synthetic surfactant (S) is known to decompose in aqueous solution according to the following reaction: S (aq)Products At 25.5°C, a 0.603 M solution of S was prepared and allowed to decompose. The reaction reached its first half life after 7 minutes. From the initiation of the reaction, the reaction reached its second half life after 10.5 minutes. Which of the following statements (i through vi) are true of the reaction at this temperature? I. The duration of the 3rd half life will be 10.5 minutes ii. The 3rd half life will be reached 12.25 minutes after the initiation of the reaction iii. The duration of the 3rd half life will be 3.5 minutes iv. Doubling the concentration of A will double the initial rate of reaction v. Doubling the concentration of A will quadruple the initial rate of reaction vi. Doubling the concentration of A will have no effect on the initial rate of reaction
Reaction of nitric oxide gas (NO) and chlorine gas (Cl2) produces a very poisonous gas called nitrosyl chloride (NOCl). The experimental data of the reaction is given below. Use the data to calculate the specific rate constant K and overall order of the reaction. Please show full work!
help a girl out?
Use the References to access important values if needed for this question. of cyclopropane to propene at 500 °C The rearrangement (CH₂)3 CH3 CH=CH2 is first order in (CH2)3 with a rate constant of 6.70 x 10- 4 S -1 If the initial concentration of (CH₂)3 is 0.141 M, the concentration of (CH₂)3 will be 0.0180 M after s have passed. Submit Answer Retry Entire Group 7 more group attempts remaining
The oxidation of ammonia produces nitrogen and water via the reaction: 4NH3(g) + 302(g) ---> 2N2(g) + 6H₂O(g). If the rate of formation of nitrogen gas is 2.0 mol/(Los), then the rate at which: water is formed is also 2.0 mol/(Los) oxygen reacts is 1.5 mol/(Los) ammonia reacts is 0.5 mol/(L •s) ammonia reacts is 4.0 mol/(Los) water is being formed is 0.67 mol/(Los)
The reaction for the decomposition of ammonia into its elements is: 2 NH3 (g) → N2 (g) + 3 H2 (g) [N2] 0.0105 M If the concentrations at a certain time are: what will be the associated value of the reaction quotient (Q)? [NH3] = 0.505 M [H2] = 0.414 M, %3D %3D (A) (B) (C) (D) (E) 0.00148 0.00292 0.00861 0.0105 342