Part AThe rate constant for a certain reaction is k = 4.60×10-³ s-1. If the initial reactant concentration was 0.700 M, what will the concentration be after 5.00 minutes?Express your answer with the appropriate units.► View Available Hint(s)[A]t =SubmitPart B[A]o =μASubmitValueA zero-order reaction has a constant rate of 4.90x10-4 M/s. If after 80.0 seconds the concentration has dropped to 1.00×10-2 M, what was the initial concentration?Express your answer with the appropriate units.► View Available Hint(s)μAUnitsValue?Units?

Rate law equation is an equation that gives the concentration of the reactant at any time t. The…

The rate constant for a certain reaction is k = 4.60x10-³ s-1 If the initial reactant concentration was 0.700 M, what will the concentration be after 5.00 minutes? Express your answer with the appropriate units. ► View Available Hint(s) [A]t = Value Submit Part B μA Submit A zero-order reaction has a constant rate of 4.90x10-4 M/s. If after 80.0 seconds the concentration has dropped to 1.00x10-2 M, what was the initial concentration? Express your answer with the appropriate units. ► View Available Hint(s) μA [A]o = Value Units ? Units ?

The rate constant for a certain reaction is k = 4.60x10-³ s-1 If the initial reactant concentration was 0.700 M, what will the concentration be after 5.00 minutes? Express your answer with the appropriate units. ► View Available Hint(s) [A]t = Value Submit Part B μA Submit A zero-order reaction has a constant rate of 4.90x10-4 M/s. If after 80.0 seconds the concentration has dropped to 1.00x10-2 M, what was the initial concentration? Express your answer with the appropriate units. ► View Available Hint(s) μA [A]o = Value Units ? Units ?

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

Consider a chemical reaction: 3 A +2B2C+2D the initial rate was measured at three different reactant concentrations. What is the rate law for the reaction? Trial 1 2 3 Initial Initial [Α] [B] (mol/L) (mol/L) (mol/(L-min)) 0.300 0.100 0.100 0.100 Initial Rate 0.100 0.200 1.35 x 10-1 1.50 X 10-2 3.00 x 10-2
The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g)+CO(g)--->CO2(g)+NO(g) The following data were collected for the above reaction Experiment No [CO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0*10-4 1.6*10-2 1.7*10-7 2 5.0*10-4 3.2*10-2 1.7*10-7 3 1.5*10-3 3.2*10-2 1.5*10-6 Determine the order of the reaction with respect to each reactant.
4. The following data were obtained for the follwing chemical reaction: 2A+38->2C+D Trial # Initial (A) Initial [B] Initial Rate of Formation (mmol/L) (mmol/L) of D (mmol/L."s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (T: 2) (b) Find the rate constant, k, with units. (T: 2)
A general reaction written as A+ 2B C+2D is studied and yields the following data: [A]o [B]o Initial A[C]/At 0.150 M 0.150 M 8.00 x 10 mol/L's 0.150 M 0.300 M 1.60 x 102 mol/L's 0.300 M 0.150 M 3.20 x 102 mol/L's What is the overall order of the reaction? O 2 03 O 4
consider the rate data at a certain temp for the reaction 2NO(g) + 2H2(g) --> N2(g) + 2H2O(g) determine the order of the reaction with respect to nitrogen monoxide
Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234
The stoichiometric equation for the reaction of nitric acid with oxygen is 2NO + O2 --> 2NO2. The following data was collected at 273°C. If the concentration of oxygen is doubled while holding the concentration of NO constant, the rate will increase by a factor of __. Experiment [NO] [O2] Initial Rate (M/s) 1 0.020 0.010 0.0320 2 0.080 0.020 1.01 3 0.040 0.040 0.50 4 0.040 0.020 0.25 5 0.030 0.010 0.71
2. 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: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
I need help filling out this table, calculating the rate law, and determining the order of the reaction