None 16. A general reaction written as A+ 2B → C + 2D is studied and yields the following data:Initial A[C]/At[A]00.150 M[B]00.150 M 8.00 × 10-³mol/L's0.150 M0.300 M 1.60 × 10-2mol/L's0.300 M0.150 M 3.20 × 10-2mol/L'sDetermine the initial rate of C production (A[C]/At) if [A] = 0.200 M and [B] = 0.500 M.a. 4.74 × 10-2mol/L'sb. 2.37 x 10 mol/L.sc. 1.19 × 10¹ mol/L.sd. 8.23 × 102 mol/L.se. None of these are correct.

To solve this problem, we need to determine the rate law for the reaction and then use it to…

Answered: 16. A general reaction written as A+ 2B…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Consider the reaction A + 2B ----> C. If the molar mass of C is twice the molar mass of A, what mass of C is produced by the complete reaction of 10.0 g A?(a) 10.0 g(b) 30.0 g(c) 60.0 g
A 0.578-g saltwater sample was titrated with 1.864 g AgNO3 solution to reach the endpoint of the reaction. Calculate the following by showing all necessary solutions: 1. mol AGNO3 if the AGNO3 solution was prepared by dissolving 5.0 g of AgNO3 in distilled water until 100 ml is reached. (MW AgNO3 = 169.87 g/mol) 2. % Cl in the saltwater sample (MM CI = 35.45 g Cl /mol CI" )
1. What is a “dNTP” and why are they included in the reaction mixture? 2. What will be the final concentration of 25 mM MgCl2, 5 mM dNTPs, and each 25 µM primer in one of the reaction tubes with the final volume of 50 microliters? Hint: use the information in the left column of Table 1 to help you with these calculations. (For one reaction) item 5.25x master mix – add things in order 32.7 µl ddH2O 171.7 µl 10 µl 5x reaction buffer 52.5 µl 3 µl 25 mM MgCl2 15.75 µl 0.5 µl 5 mM dNTPs 2.63 µl 1 µl 25 µM “forward” primer (#3012) 5.25 µl 1 µl 25 µM “reverse” primer (#3013) 5.25 µl 0.8 µl thermostable polymerase 4.2 µl (do not add until needed) Total: 49 µl Total: 257.3 µl
A certain first order reaction has the rate law Rate = k[A] with k=0.0068 sec-1. If the initial concentration of A is 0.75 M, what will be the concentration of A after 1 minute? What is the half-life for this reaction? How much time will it take for 75% of A to react? How much A will be left after the passage of three half-lives? What is the initial rate of the reaction?
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For the reaction E + S ES, what is the [E] if [S] = 0.18 mM, [ES] = 133 uM, and the Kd = 15 uM? 11,000 UM 20 uM 11 uM O 180 UM
ver is given. A +B C+ D 1) Calculate AG for the above react un and indicáte whether the reaction is favorable or unfavorable [A] = 0.9 M 20°C AG° = 4 KJ/mol %3D [B] = 15mM [C] = 4mM [D] = 3 M R= 8.314 J/moleK %3D %3D 4.7 and explain how you know.
For the following reaction X + YA + B at 300 K, it is found equilibrium constant equal to 10. Therefore, AG & AGⓇ of the reaction at 300 K respectively are - Answer b
The Ksp values of silver chromate Ag2CrO4 and silver iodate Ag(IO3) are given below. Ag2CrO4 Ag(IO3) Ksp 1.12 x 10-12 3.17 x 10-8 Based on these Ksp values, which of the following is true? Choose one option only. Options: a. In the solution consisting of 1.00 x10-4 M Ag+ and 5.00 x10-5 M CrO42-, Ag2CrO4 precipitate will form. b. In the solution consisting of 1.0 x10-4 M Ag+ and 1.0 x10-4 M IO3-, Ag(IO3) precipitate will form. c. In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3). d. In the solution consisting of 0.200 M CrO42- and 0.200 M IO3-, Ag2(CrO4) will precipitate first if we add Ag+ ions gradually into the above mixture.
3. Show the calculation of (1) the expected grams of alum (KAI(SO4)2 12 H2O) formed from the reaction of 1.4 grams of aluminum metal and then show the calculation of (2) the % yield if the actual yield of alum is 21.31 grams. Overall reaction is shown below: 2 Al + 2 KOH + 10 H2O + 4 H2SO4 →2 KAI(SO4)2 12 H2O + 3 H2(g)T
The reaction quotient is Q=1.6×10-26 Part B What pH is needed to produce this value of Q if the concentration and pressure values are [Br2]=2.50×10−4M , [Br−]=11.65M, [SO42−]=9.50M, and PSO2=3.50×10−5atm ? Express your answer numerically to two decimal places.
Ethylene oxide is produced industrially from the reaction of ethylene with oxygen at atmospheric pressure and 277 oC, in the presence of silver catalyst.C2H4(g) + O2(g) → C2H4O(g) (unbalanced)Assuming 100 % yield, how many kg of ethylene oxide can be produced from 34600 L of a mixture containing ethylene and oxygen in 1:1 molar ratio?

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