A reaction is Oth order in reagent B. The rate of the reaction is 3.5 x 10 3 M/sec when the concentration of B is 0.50 M. How much B remains 100 seconds later? Selected Answer: 0.35 M а. Answers: 0.35 M a. 0 M, all the B is consumed. b. 1.04 M C. 0.85 M d. 0.15 M e.

A reaction is Oth order in reagent B. The rate of the reaction is 3.5 x 10 3 M/sec when the concentration of B is 0.50 M. How much B remains 100 seconds later? Selected Answer: 0.35 M а. Answers: 0.35 M a. 0 M, all the B is consumed. b. 1.04 M C. 0.85 M d. 0.15 M e.

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU5: Fire: Energy , Thermodynamics, And Oxidation-reduction

SectionU5.13: Speed Things Up: Rate Of Reaction

Problem 1TAI

See similar textbooks

Similar questions

Pls help ASAP. PLS look at the diagram of the graph to answer this.
Please explain how to find rate constant (k) if reaction rate = 3.40*10^-7 I^- molar = .00200 (reaction order 1) BrO3^- molar = .00800 (reaction order 1) H^+ molar = .0400 (reaction order 2)
I-(aq) + OCI-(aq) 10-(aq) + Cl-(aq) The above reaction was studied (at a particular temperature) and the following data were obtained: [1-10 [OCI-]0 Initial Rate (mol/L) (mol/L) (mol L-1s-1) 0.360 0.100 8.42\times 10-20.045 0.100 1.05\times 10-20.090 0.200 4.21\times 10-20.180 0.200 8.42\times 10-2 Which of the following expressions for the rate law are completely consistent with the above experimental data, d[Cl-]/dt = kl OCI-][-] d[10-]/dt = k[OCI-]3 k[OCI][I] = d[OCI-]/dt-d[-]/dt = k[-]2[OC]d[1]/dt = k[-][OC] 1 pts Tries 0/5 Calculate the rate constant (k). (Units required.)
answer all parts please!
Please correct answer and don't use hend raiting
Fast pls i will give u like for sure solve this question correctly in 5 min i will give u like for sure The reaction rate between 6 s and 10 s is V = _______________ = -d[A]/second. (use 2 sig figs) The rate constant is k = ___________________(use units of s-1 and/or M-1 as needed, round to 2 sig. figs).
I included my data table please answer the following questions Find the delta(S2O8^2-),M (2nd to last row on data table), THEN find the Reaction rate for all 4 runs (last row). IGNORE THE NUMBERS THAT ARE IN THOSE COLOUMNS RIGHT MOW THEY ARE MOST LIKELY INCORRECT! Next find the average rate consant k for the 4 runs using the numbers you calculated.
pdf is needed, but algebra & For an instantaneous rate of change, is used to denote geometry can be used to approximate the value. The symbol an instantaneous change in a value, 1) What is true about the reactant concentration over time? A[Reactant] constant? At d[Reactant] 3) Circle the time at which the magnitude of the (instantaneous rate of dt change) is the lowest (i.e., during which time is the tangential slope least negative? This is the time when the [reactant] is changing least over time) 0.20 Concentration of reactant vs time 0.15 Rate = -Slope = 1.06x10-2 M/sec jou 0.10 0.05 0.00 15 10. Time, sec. 20 25 https://wnww.chem.purdue.edugdhelphowfosolveilKineticsCalculaingRales.html
Experimental data shows the rate order of [A] is second order. (a) This means as [A] doubles, the reaction time _____. A. is quartered B. increases by a factor of eight C. is cut in half D. doubles (b) This means as [A] is cut by a third, the reaction time _____. A. is decreased by a factor of three B. triples C. is decreased by a factor of six D. increases by a factor of nine
PERTINENT CALCULATIONS Remember: rate = k[C25H30CIN3]"[OH_]" where n =0 since excess OH was used. n3= 1. Refer to your graphs and complete table below Linear correlation (r- value) Graph Kinetic Run I Kinetic Run II Average r- value absorbance vs time 0.9972 0.9955 0.9964 In (absorbance) vs time 0.9978 0.9994 0.9986 2/(absorbance) vs time 0.9805 0.9879 0.9952 2. Based on the average linear correlation (r2 -value) the reaction order, m, with respect to crystal violet, CV, is Explain. 3. Write the rate law. 4. The slope, and therefore pseudo" rate constant, kr', is at T1. CC, and ko' is at T2
Choices.. 1 A. R for 1st order a. -0.999 B. -0.988 C. 0.988 D. 0.969 B. R for 2nd order a. -0.999 B. -0.988 C. 0.988 D. 0.969 2. Order a. 1st b. 2nd 3. Rate constant a. 1.84 x 10^-3 b. 179.97 c. 5.43 x 10^-3 d. 7.20 x 10^-4 4. HI concentration a. 0.893 b. 12.40 c. 2.44 d. 2.43 x 10^5
Assistance completing worksheet