MISSED THIS? Watch KCV 14.3. IWE 14.1: Read Section 14.3. You can click on the Review link to access the section in your eText Consider the reaction: A(g) + B(g) →2C(g). identify the expression for the rate of the reaction with respect to each of the reactants and products Part B rate= -- AA rate= -2 rate=- Submit AB O rate= -24 23 == AA Request Answer 1 AB 1 AC 2 At 11 = AC At AC At AB AC At When C is increasing at a rate of 4.0x102 M-s, how fast is B decreasing? Express your answer using two significant figures. ΜΕ ΑΣΦ ? M-s-¹

MISSED THIS? Watch KCV 14.3. IWE 14.1: Read Section 14.3. You can click on the Review link to access the section in your eText Consider the reaction: A(g) + B(g) →2C(g). identify the expression for the rate of the reaction with respect to each of the reactants and products Part B rate= -- AA rate= -2 rate=- Submit AB O rate= -24 23 == AA Request Answer 1 AB 1 AC 2 At 11 = AC At AC At AB AC At When C is increasing at a rate of 4.0x102 M-s, how fast is B decreasing? Express your answer using two significant figures. ΜΕ ΑΣΦ ? M-s-¹

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...

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* Question Completion Status: A Moving to another question will save this response. Question 18 The mechanism for NO2 (g) + CO (g) → NO (g) + CO2 (g) is thought to be: 2 NO2 → NO3 + NO NO3 + CO → NO2+ CO2 (slow) (fast) The rate law for the overall reaction is: Rate = k[NO3][CO] O Rate = k[NO2] Rate = k[NO2]2 O Rate = k[NO2][CO] O Rate = k[NO3][NO] A Moving to another question will save this response. MacBook Air 吕0 F6 esc F3 F4 F5 F1 F2 #3 $4 % 3 4. 6. 回2 Breathe easy
Consider the reaction: A -----------> 2C The concentration of reactant A and product B were monitored at the same time interval. Time t, Minutes Molar Concentration A, [A] Molar Concentration C, [C] 0 2.40 0.00 2.00 2.20 0.40 4.00 2.00 0.80 Identify the correct rate of the reaction. 0.00 0.40 0.80
A certain reaction is first order in H, and first order in I,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [4.] [+] initial rate of reaction Calculator 圖 х10 0.429 M 0.563 M 0.0218 M/s olo 0.429 M 1.36 M |M/s 18 Ar I M/s 0.0981 M 2.46 M
50. The tabulated data were collected for this reaction: 19mmlich CH3 Cl(g) + 3 Cl₂(g) → CCl4 (g) + 3 HCl(g) [CH3CI] (M) 0.050 0.100 0.100 0.200 [Cl₂] (M) 0.050 0.050 0.100 0.200 ME Initial Rate (M/s) 0.014 0.029 0.041 0.115 Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?
Initial rate data at a certain temperature is given in the table for the following reaction. [NOCI], (M) Initial rate of formation of Cl, (M/s) 2 NOCI(g) → 2 NO(g) + Cl, (g) 0.600 1.30 x 10-5 0.750 2.03 x 10-5 0.900 2.92 x 10-5 Determine the value and units of the rate constant, k. Units: k :
The reaction 2NO(g) + Cl2 (g) -----> 2NOCl (g) was studied at –10°C. The following results were obtained where Rate = - Delta [Cl2]/ delta t [NO]0 [Cl2]0 Initial Rate (mol/L) (mol/L) (mol/L·min) 0.11 0.11 0.24 0.11 0.22 0.48 0.22 0.22 1.92 a Question Content Area What is the rate law? ( Use k for the rate constant. ) Rate =
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.
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or a reaction involving two reagents A and B, the following data was collected over three experiments. Exp# [A] [B] Rate (M/s) 1 0.20 M 0.20 M 5.0 2 0.20 M 0.40 M 20.0 3 0.10 M 0.40 M 10.0 Using the above data, which of the following is the rate law for the reaction of A with B?
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] 3.4 3.4 1.223775 0.294118 25 2.28 0.824175 0.438596 2.822 + 50 1.53 0.425268 0.653595 2.244 + 75 1.02 0.019803 0.980392 1.666 - 1.088 - 0.51 - 15 30 45 60 75 t y=-0.03156 x + 3.241000 2= 0.971 Add Row 10 total rows What is the reaction order? O 1 Calculate the concentration of A after 127 s. [A]127 s = M [V)
Consider the reaction between nitric oxide and hydrogen 2NO + H2 → N20 + H20 Initial Rate of Disappearance of NO Experiment Initial [NO], M Initial [H2], M (mol/L sec) 1 6.4 x 10-3 2.2 x 10-3 2.0 x 10-5 2 12.8 x 10-3 2.2 x 10-3 8.0 x 10-5 6.4 x 10-3 4.4 x 10-3 4.0 x 10-5 What is the rate law for this reaction? a. Rate = k[NO] b. Rate = k[NO]? c. Rate = k[NO]²[H2] d. Rate = k[No][H2]