2 NO(g) + Cl2(g) → 2 NOCl(g) Initial Rate (M-min-1) 0.18 0.36 1.45 Exp. # |...
The reaction between nitric oxide (NO) and chlorine (Cl2) to form nitrosyl chloride (NOCl) was found to occur as an elementary reaction as follows: 2 NO (g) + Cl2 (g) à 2 NOCl (g) A table of the concentrations and initial rates data is shown below: [ NO ]0 (M) [ Cl2 ]0 (M) rate = - D[Cl2]/ Dt (M / min) Run 1 0.10 0.10 0.18 Run 2 0.10 0.20 0.36 Run 3 0.20 0.20 1.44 The order for Cl2 in this reaction is: (a) 1 (b) 45 (c) 2 (d) 180
The reaction 2N0(g) + C12(g) --+2NOCl(g) was studied at 1o°C. The following results were obtained where Δ[C12] Rate Initial Rate (mol/L-min) INOlo (mol/L) [Clalo (mol/L 0.10 0.10 0.20 0.10 0.20 0.20 0.18 0.36 1.45 a. What is the rate law? b. What is the value of the rate constant? (2) The rate law for the reaction at some temperature is: NOBr a. If the half-life for this reaction is 2.00 s when [NOBro 0.900 M, calculate the value of k...
For the reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) a possible mechanism is (1) NO + Cl2 ⇆ NOCl2 fast (2) NOCl2 + NO → 2 NOCl slow What is the rate law for this mechanism? (Enter an answer in the form k[A][B]^2^, where the appropriate chemical species replace A and B, and the correct orders are indicated.) Enter a formula by surrounding subscripts with underscore "_" and superscripts with carat "^" characters. For example, H3O+ would be entered...
NOCl decomposes by the following reaction: 2NOCl (g) --> 2 NO (g) + Cl2 (g). THe table below is collected at the same temperature. Time (s) 0 10 20 30 40 [NOCl] 0.0800 M 0.0606 M 0.0488 M 0.0408 M 0.0350 M how would you find the rate law for this reaction and what is the rate law? also what is the concentration of NOCl after 60 seconds?
Consider the hypothetical reaction: 2 X + Y → Z and its general rate law Rate = k[X]m[Y]n The following data was obtained when the reaction studied at –10°C: [X], M [Y], M Rate, M/min 0.10 0.10 0.18 0.10 0.20 0.36 0.20 0.20 1.45 (a) What is the order of reaction with respect to X? (2 points) (b) What is the order of reaction with respect to Y? (2 points) (c) What is the overall order of reaction?...
2NO (g) +Cl2 (g) → NOCl (g) Experiment concentration of NO (M) concentration of Cl2(M) Rate (M/s) 1 0.05 0.01 3.40 x 10-4 2 0.025 0.01 8.50 x 10-5 3 0.025 0.04 3.40 x 10-4 What is the reaction order with respect to NO ? the reaction order with respect to reaction order to Cl2 ? overall reaction order ? what is the rate constant ?
What is rate law? exp# [A](M) [B](M) (M/min)Initial Rate 1 1. 2.50 20. 2 3. 5. 360. 3 1. 5. 40. 3
lthe system 2NO (g) +Cl2 (g) <-----> 2 NOCl (g) has a Kc= 6.5x10^4 at 35°C. determine which direction will the system shift (forward or backward) if it has these initial concentrations: [NO]0 =0.0275 M, [Cl2]0 =0.0384 M, [NOCl]0 =1.750 M.
A Review | Constants | Periodic Table You place 1.45 mol of NOCl(g) in a reaction vessel. Equilibrium at constant pressure is established with respect to the decomposition reaction Part C Calculate NOCI(8) = NO(g) + Cl2 (8) AGE and the degree of dissociation of NOCl in the limit that is very small at 350. K and a pressure of 1.50 bar. AH Substance (kJ · mol-1)(298 K) (kJ. mol-1)(298 K) NOCI(g) 51.7 66.1 NO(g) 91.3 87.6 Cl2 (g) 0...
2NO(g) + Br2(g) = 2NOBr(g) Experiment [NO-] (M) [Br2] (M) Initial Rate (M s-1) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 1.) Determine the rate law equation for the reaction. 2.) What is the overall order of the reaction? 3.) What are the value and the units of the rate constant, k? 4.) Write the expression to show how is the rate of disappearance of bromine, Br2, related to the rate...