The decomposition of N»Os(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is:A[N,05]Rate= *[N,Os]Atwhere k = 3.4 x 10-5 s-l at 25°C, what is the initial rate of reaction at 25°C where [N2O5]o = 4.1 x 10-2 M?а. 1.4x 10-6 mol/L'sb. 3.4 x 10-5 mol/L'sО с. 8.3 х 10-4 mol/L sd. 4.1 x 10-2 mol/L'se. none of these

Given : Reaction is first order with respect to reactant N2O5. Rate constant = 3.4 X 10-5 s-1 And…

The decomposition of N,Os(g) to NO>(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,05] = k[N,O;] Rate = At where k = 3.4 x 10$ s' at 25°C, what is the initial rate of reaction at 25°C where [N,O5lo = 4.1 x 10² M? a. 1.4 x 10-s mol/L's O b. 3.4 x 10-5 mol/L's O c. 8.3 x 104 mol/L-s O d. 4.1 x 10-2 mol/L•s e. none of these

The decomposition of N,Os(g) to NO>(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,05] = k[N,O;] Rate = At where k = 3.4 x 10$ s' at 25°C, what is the initial rate of reaction at 25°C where [N,O5lo = 4.1 x 10² M? a. 1.4 x 10-s mol/L's O b. 3.4 x 10-5 mol/L's O c. 8.3 x 104 mol/L-s O d. 4.1 x 10-2 mol/L•s e. none of these

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

For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
Give only typing answer with explanation and conclusion The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A]. Assume k = 8.82 x 10-4 s-1 . If the initial concentration of A is 1.44 mol L-1, what is the concentration of A (in mol L-1) after 97.6 minutes?
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.27/s. Fe3+(aq) + SCN-(aq) → Fe(SCN)2+(aq). How many seconds would be required for the initial concentration of Fe3+ to decrease to 12.5% of its initial value? Express your answer to two decijal positions.
For the given equation at 800 °C: CO(g) + Ch(g) > COCh(g), the following data were collecica Experiment (COL(M) 0.96 1.92 0.96 (CH] (M) 1.60 1.60 3.20 Rate of appearance COCh (M/s) 0.121 0.242 0.484 Determine the Rate Law for the reaction From your Rate Law determined in question #1 above, determine the value of the rate constant WITH THE APPROPRIATE UNITS. ONLY If you could not answer #1 above, use this "mock" data to solve for k: Rate = K[ARB]?, with [A] = 1.00 M and B]o = 1.50 M, with a rate of 2.50 x 10-2 M/s.
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) is zero order in HI with a rate constant of 1.20×104M s!. If the initial concentration of HI is 0.103 M, the concentration of HI will be 1.33×10-2 M after seconds have passed.
Consider this reaction: 280; (g) → 2S0, (g) +0, (g) At a certain temperature it obeys this rate law. rate =(3.43 s")[so,] S SO Suppose a vessel contains SO, at a concentration of 0.590M. Calculate the concentration of SO, in the vessel 0.320 seconds later. You may assume no other 3 reaction is important. Round your answer to 2 significant digits. х10
1) Please help
Consider this reaction: 2H,PO, (ag) – P,0, (aq)+ 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (0.392 M-1.s Suppose a vessel contains H, PO, at a concentration of 0.520 M. Calculate how long it takes for the concentration of H, PO, to decrease to 12.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
Don't give handwritten answers otherwise I will dislike
Consider this reaction: 2C1,0, g) → 2C1, (6) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.36 Ms)[C1,0,1 %3D Suppose a vessel contains Cl,0, at a concentration of 0.630 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.