Question 1 In a particular study of the reaction described by the equation, 2 CH40(g) + 3 02(g) → 2 CO2(g) + 4 H20(g) the rate of consumption of CH40(g) is 0.480 M s-1. What is the rate of consumption of O2(g) in the study? OA0.72 M s-1 O B. 1.4 Ms-1 OC. "0.32 M s-1 OD-0.48 M s-1 OE 0.24 Ms-1 OF 3.1 Ms-1

Question 1 In a particular study of the reaction described by the equation, 2 CH40(g) + 3 02(g) → 2 CO2(g) + 4 H20(g) the rate of consumption of CH40(g) is 0.480 M s-1. What is the rate of consumption of O2(g) in the study? OA0.72 M s-1 O B. 1.4 Ms-1 OC. "0.32 M s-1 OD-0.48 M s-1 OE 0.24 Ms-1 OF 3.1 Ms-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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Smail ||| YouTube O KINETICS AND EQUILIBRIUM Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 0.0108 s NH,OH(aq). } → NH, (aq) +H,O(aq) Translate M Suppose a vessel contains NH4OH at a concentration of 1.24 M. Calculate the concentration of NH OH in the vessel 63.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation 82°F Mostly cloudy Check 0/5 Q Search © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | 1
Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, A. Which is the rate law of this reaction? B. which is the numerical value of the specific-rate constant, k, for this reaction? C. Which are the units for the specific rate constant, K? D. At whic rate is T generaten when [T2U] is 0. 111 M? E. if given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed?
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Consider Following reaction: CH4(g) + 4 NO(g) → 2 N2(g) + CO2(g) + 2 H2O(g) The concentration of NO was 3.176M at t = 0.39 s and 0.947 M at t = 7.60 s. What is the rate of consumption of CH4 in M/s? Report your answer with four decimals. Enter numbers only; do not enter units.
H₂O₂(aq) +31 (aq) + 2H*(aq) →→ 13¯(aq) + 2H₂O(l) If the concentration of I drops from 1.045 M to 0.760 M in 10.7 seconds, what is the rate of disappearance of H*? 7.99x10-2 MS1 1.78x10-2 MS-1 5.33x10-2 MS-1 2.66x10-2 MS1 4.00×10-² MS-1
Question 9 of 36 Submit What is the rate at which Br"(aq) disappears in the reaction below if the rate of disappearance of BrO3 (aq) is 0.020 M/ s? BrOg + 5 Br + 6 H* → 3 Br2 + 3H20 | M/s 1 2 3 4 C 7 9 +/- х 10 0 LO 00
2NOCl(g) → 2NO(g) + Cl2(g) Rate = k[NOCl]2If this gaseous system has an initial rate of decomposition of NOCl of 0.0010 M s-1, and the volume of the system is reduced to one fifth of its original value, what is the new initial rate of decomposition of NOCl? Assume the temperature remains the same. 5.0×10-3 M s-1 2.5×10-2 M s-1 2.0×10-4 M s-1 4.0×10-5 M s-1 1.0×10-1 M s-1
A: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate of Zn2+ formation if its concentration rises from 0.00 to 0.069 M in 2 minutes and 12 seconds? Group of answer choices 0.031 M/s 2.1 x 10-3 M/s 1.3 x 10-4 M/s 5.2 x 10-4 M/s B: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min
A Moving to another question will save this response. Question 24 The rate law for the reaction below is rate = k[N21*[H2]Y 2 NH3 N2 + 3 H2 - Which of the following is true? OA.x = 3 and y = 1 OB. The reaction is 4tn order overall OC The order of reaction needs to be determined experimentally O D.X = 1 and y = 1 OE.x = 1 and y = 3 A Moving to another question will save this response. MacBook esc F1 F2 F4 FS 23 3 4. tab aps lock F
2A B For the reaction above, what is the average rate of a reaction over the first 100 seconds if the reactant disappears according to the following table? 3 Time(s) [A] (M) 0.0 1.3 50.0 1.0 100.0 0.84 150.0 0.5 200.0 0.2 250.0 0.1 E D Your Answer: KO 4 Answer OE R F 96 5 T G 6 B units 4- & H 7 99- N #0 bp U J 8 M T 9 K 44 P - alt { ? ? + + [ H 7 H 77°F ^ insert } ← ctri ( pause 9:43 PM 9/13/2022 prt sc backspace delete enter home T shift pg up pg dn end (intel PENTIUM GOLD
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. ?
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