battery lifeSee disclaimers on product box Battery ife wl vary depending on various factors Inclproduct model, comfguration, loaded appications, features, use, wireless functionatity,Dower management settings. The madmum tapady of the battery wil naturaly decremsetime and usage. see bapca.com/products/mobilemark-2014.25°C. If the initial concentration of Mn(CO)s is 1.0 × 10$M, how long will it take for 90.% of the reactant9. The second-order reaction, 2 Mn(CO)s → Mn2(CO)10 has a rate constant equal to 3.0 x 10° M's atto disappear?

The integral rate equation for the 2nd order reaction is; t=1k1MnCO5t-1MnCO50

9. The second-order reaction, 2 Mn(CO)s → Mn2(CO)10 has a rate constant equal to 3.0 x 10° M's at 25°C. If the initial concentration of Mn(CO)s is 1.0 × 10 M, how long will it take for 90.% of the reactant to disappear?

9. The second-order reaction, 2 Mn(CO)s → Mn2(CO)10 has a rate constant equal to 3.0 x 10° M's at 25°C. If the initial concentration of Mn(CO)s is 1.0 × 10 M, how long will it take for 90.% of the reactant to disappear?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 105QAP: Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a)...

See similar textbooks

Related questions

Q: The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second-order…

A: Rate of reaction is directly proportional to the initial concentration of the reactant…

Q: Certain organic molecules can undergo dimerization. Butadiene when it undergoes this type of…

Q: hydrogen iodide decomposes according to the equation shown below. The second-order rate constant for…

Q: If the instantaneous reaction rate for the reaction given below was 2.11 x 10-7 M/s when the…

A: [Br2] = 0.0332 M [H2] = ?

Q: The reaction of butadiene gas (C4H6) to yield C8H12 gas is described by the equation: 2 C4H6(g)…

A: Recall the "dimerization" reaction of butadiene C4H6 - 2 C4H6 g → C8H12 gThe…

Q: Part A The first-order decomposition of N,Os at 328 K has a rate constant of 1.70 x 103 s1, If the…

A: Given: Rate constant, k = 1.70 x 10-3 s-1 Initial concentration [N2O5] = 2.88 M t = 12.5 min = 750 s…

Q: 8. The reaction A(g) → 2B(g) has a rate constant k = 3.6 x 10/second. a) Is the reaction zero order,…

A: Given: A(g) =2B(g) k = 3.6 x 10-3 s-1 a) Observe the unit of the given rate constant value.

Q: 7. Hydrogen peroxide decomposes into water and oxygen gas by a zero-order process. The rate constant…

A: The integrated rate law for the zero-order reaction A → products is [A]t = [A]0 - kt Because this…

Q: A second-order reaction starts with an initial concentration of 0.5 mol/L of the reactant. If the…

A: Given data contains, Initial concentration of the reactant is 0.5 mol/L. Final concentration of the…

Q: The rate constant, k, for a first-order reaction is equal to 3.60 × 10-5 s-1. What is the half-life…

Q: 3 4 1 5 6 7 8 At a certain temperature the rate of this reaction is first order in HI with a rate…

A: Given, 2HI(g) ➝ H2(g) + I2(g) The reaction is first order Kinetic. Rate constant (k) = 0.0797 s-1…

Q: The first-order decomposition of cyclopropane has a rate constant of 6.7 x 10-4 s-1. If the initial…

Q: 20 Molecular bromine, Br2 (g) dissociates into bromine atoms at 625 K with a first-order rate…

Q: Chemists graph kinetic data to determine rate constants and the order of reactions. Analyze this…

A: Ans The given rate constant for the rate constant K= 0.019Ms-1 Standard units for rate constant K =…

Q: The reaction 2NO2⟶2NO+O2 has the rate constant k=k= 0.63 M^−1s^−1 Part A: Based on the units for k,…

A: A) The units of rate constant is given M-1 s-1 Assuming the rate of reaction = K X [NO2]n where…

Q: The decomposition of nitrosyl bromide at 10 °C NOBrNO + ½ Br2 is second order in NOBr. In one…

A: Given Initial concentration of NOBr 0.424 M concentration of NOBr dropped = 7.46×10-2 M Time = 9.21…

Q: The rate constant for a first-order reaction is 0.54 s¬1. What is the half-life of this reaction if…

A: • The values provided in the question are:- i) Rate constant of a first order reaction, k1 =…

Q: 2) A first order process has an experimentally determined rate constant of 6.0 x10 s' at 500°C. If…

Q: The reaction of butadiene gas (C4H 6 ) with itself produces C8H 12 gas as follows:…

Q: The reaction SO,Cl2 (g) --> SO2 (g) + Cl2 (g) is first order. At 660 K it has a rate constant of 4.5…

A: First order reaction. Rate constant = 4.5 × 10-2 s-1 time = 18.9 seconds Initial concentration =…

Q: The reaction rate constant for a particular first order reaction is .820 M/s. How many seconds will…

Q: 11 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In…

Q: The conversion of cyclopropane to propene in the gas phase is a first-order reaction with a rate…

A: In chemical kinetics, the reactions are classified on the basis of their order. In first order…

Q: NO2Cl(g) + NO(g) -----> NO2(g) + ONCl(g) A is 8.3 x 108 and Ea is 28.9 kJ/mol. The rate equation is…

Q: The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 x10-4/s at 45…

Q: The rate constant for a certain reaction is k = 8.80×10−3 s−1 . If the initial reactant…

A: From the unit of rate constant we can say that it is first order equation

Q: (6a) The gas phase decomposition of nitrosyl chloride at 400 K NOCl(g)NO(g) + ½ Cl2(g) is second…

Q: At a given temperature, a first-order reaction has a rate constant of 3.5 x 10-3s How long will it…

A: Here given, Rate constant for the first order reaction (k) = 3.5×10-3 s-1 We have to calculate the…

Q: The rate constant for this first-order reaction is 0.0251 s−1 at 300 °C. A⟶products If the initial…

A: The integrated equation for first order reaction is expressed as :

Q: Consider the reaction A + 2B à C The rate law for this reaction is second order in A and second…

A: Rate of a reaction is the speed at which the reaction proceeds or the reactants getting converted…

Q: The decomposition of nitrogen dioxide gas (NO,) to nitrogen monoxide (NO) and oxygen(0,) gases is a…

A: By applying second order rate kinetics, we can find rate constant.

Q: The decomposition of NO2 is a second order reaction and the rate constant is 0.755 L/mol-s. In an…

Q: Can you please help me identify which is which !

A: The order of each reactant in a reaction is represented by the exponential term of the respective…

Q: (16. A reaction that is second-order in one reactant has a rate constant of 2.2 x 10 L/(mol s). If…

A: Given, Reaction of second order, Rate constant (K) = 2.2 × 10-2 L/mol•s Initial concentration of the…

Q: The rate constant for this first‑order reaction is 0.910 s−1 at 400 ∘C. A⟶products How long, in…

A: First-order reaction: The rate of the first-order reaction depends only on one reactant. According…

Q: The second-order rate constant for the decomposition of ClO is 6.63×109 M–1s–1 at a particular…

Q: The reaction of butadiene gas (C4H6) with itself produces C8H12 gas as follows:…

A: The integrated rate law for the 2nd order reaction is given by, kt = 1[A]-1[A]0 where k is the rate…

Q: The decomposition of NO2 is a second order reaction and the rate constant is 0.755 L/mol-s. In an…

A: t = time required to concentration of NO2 to drop to 0.00100 mol/L

Q: (Q89) The hydrolysis of sucrose to form fructose and glucose is a first order reaction that has a…

A: Initial concentration of sucrose = 0.879M Final concentration of sucrose = 0.363M Half life time =…

Q: The rate constant for a second-order reaction was determined as 0.186 L mol-1 s-1. How long does it…

A: Given Initial Concentration (A)0 = 0.0671 M Remaining Concentration (A) = 0.0125 M Rate…

Q: The rate constant of a first-order reaction is 4.60 x 104 s at 350 degrees Celsius. If the…

A: First order reaction is a reaction in which the rate of the reaction is dependent upon the…

Q: The rate constant for the decomposition of HI(g) forming 2(g) and H2(g) at 700 °C was found to be…

A: '

Q: 16 The reaction C2H5Cl →C2H4 + HCl is first order in C2H5Cl. The rate constant is 1.60 x 10-6/s. In…

Q: 3(a) Substance A reacts according to a first order rate law with k = 5.0 x 10-5 s-1 3(a)(i) If the…

A: Using first order reaction integrated rate law , we will calculate rate.

Q: 15. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second-order…

A: The reaction is second order with respect to NO and First Order with O2 then, RATE= K*[NO]2[O2]…

Q: The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second-order with…

A: GIven, [NO] = 0.025M [O2] = 0.015M

Q: If a reaction involving a single reactant is first order, with a rate constant of 4.50 x 102 s1, how…

Question

battery life
See disclaimers on product box Battery ife wl vary depending on various factors Incl
product model, comfguration, loaded appications, features, use, wireless functionatity,
Dower management settings. The madmum tapady of the battery wil naturaly decremse
time and usage. see bapca.com/products/mobilemark-2014.
25°C. If the initial concentration of Mn(CO)s is 1.0 × 10$M, how long will it take for 90.% of the reactant
9. The second-order reaction, 2 Mn(CO)s → Mn2(CO)10 has a rate constant equal to 3.0 x 10° M's at
to disappear?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a cell.
What is wrong with the following statement: The best concentration cell will consist of the substance having the most positive standard reduction potential. What drives a concentration cell to produce a large voltage?
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.