For the reaction 4 CH, CH₂(g) +14 NO₂(g) →7N₂(g) + CO₂(g) 12H₂O(g), the rate of the reaction in terms of the change in nitrogen dioxide concentration would be written as: O a) 144[0] A[NO₂] Ob)[0] Od -14 A[NO₂] At Od) _A[NO₂] At Oe) - A[NO₂] *

For the reaction 4 CH, CH₂(g) +14 NO₂(g) →7N₂(g) + CO₂(g) 12H₂O(g), the rate of the reaction in terms of the change in nitrogen dioxide concentration would be written as: O a) 144[0] A[NO₂] Ob)[0] Od -14 A[NO₂] At Od) _A[NO₂] At Oe) - A[NO₂] *

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

The synthesis of ammonia obeys the following reaction: N2(g) + 3H2(g) → 2 NH3(g) N2(g) concentration measurements were taken at different times and plotted. 1) What is the average reaction rate of NH3(g) between 0 and 3 hours? (Attention, the graph is in "hour" and we want a speed in "mole/L s") 2) What is the instantaneous rate of reaction of NH3(g) at the 1st hour? 3) What is the general speed between 0 and 3 hours?
3ClO- → ClO3- + 2Cl- If the rate of formation of ClO3- is 1.2 × 10-4 M s-1, what is the rate of disappearance of ClO-?
I am unclear how to order a reaction
See image below. Can you please show me how to solve this problem?
A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H, initial rate of reaction х10 1.26 M 0.560 M 76.0 M/s | M/s 1.26 M 0.272 M | M/s 5.70 M 0.124 M
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
Consider the reaction A + 2B = C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [A] [B] (M) (M) 0.20 0.010 4.8x10-4 2 0.20 0.020 9.6x10-4 3 0.40 0.010 1.9x10-3 Trial 1 Rate (M/s) What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B].
Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Write 2-3 sentences to describe how you determined the rate law for the reaction.
A certain reaction has the following rate law: rate = k[X]³[Y]² Which of the following are the correct units for k? Select one: L³mol-3s-1 Ms-1 M³s O L?mol2s1 L5mol 5s1 Lmol-'s mol³L-3s-1 M's-1 L*mol-4s-1 mol?L-2s1
Ln [A] Post Lab Assignment 1. Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl, (g) Determine the rate law, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) Rate (mol L-1 h-1) 0.10 0.20 0.30 3.2 x 10-9 7.2 x 10-9 2. A 5.0 mL dye solution of 3.45 e-5 M is mixed with 15.0 mL bleach solution of 0.21 M. What are the initial concentrations of [Dye] and [Bleach] for your experiment? 3. The plots of 1/[A] vs time, In([A]) vs. time, and [A] vs. time of a solution of substance A are shown below. What is the reaction order with respect to A? 000 009 007 000 0 20 40 Time (min) Time 09 08 Time
Consider the balanced chemical equation. H₂O₂ (aq) +31 (aq) + 2H+(aq) → I3¯¯(aq) + 2H₂O(1) In the first 11.0 s of the reaction, the concentration of I drops from 1.000 M to 0.752 M. Part A Predict the rate of change in the concentration of H₂O2 (A[H₂O2]/At). Express the rate to three significant figures and include the appropriate units. A[H₂O₂]/At = Submit Request Answer Part B Value μÀ HÅ Δ[13]/Δt = Value Predict the rate of change in the concentration of I3 (A[13¯]/At). Express the rate to three significant figures and include the appropriate units. Submit Request Answer Units Units ? www. ?
Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction? A) [B] = [B]₀ - kt B) [B] = [B]₀ × e^(-kt) C) 1/[B] = 1/[B]₀ + 2kt D) All of the above