Homework Answers
3) K1 is the pseudo-rate constant for the reaction. That means reaction looks like perticular order but original order of the reaction may be different. This is because the rate of the reaction might not be depend on concentration of one of the reactants. Hence true rate constant is different from rate expected.
Hence true rate constant is different from pseudo-rate constant.
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Technically, k' is a pseudo-rate constant. Explain why k' is not the true rate constant for...
3. Determine a value of the pseudo-order rate constant, kobs. What is the half-life of the...
3. Determine a value of the pseudo-order rate constant, kobs. What is the half-life of the reaction under the conditions of the experiment? For how many half-lives was the reaction allowed to run? C9H8O4 + NaOH -------> C9H7O4Na + H2O Concentration of C9H8O4 = 5x10-4M NaOH = 7.1x10-5M **Second order reaction in respect to acetylsalicylic acid. **The rate law may be written as, rate = k[asp]m[OH– ]n and The pseudo-rate law is rate = kobs[asp]m Where kobs = k[OH– ]n...
Can someone please explain the equilibrium rate constant and what it means and why it is used her...
Can someone please explain the
equilibrium rate constant and what it means and why it is used
here, and how it relates to the k and k prime shown above. Thank
you!
How is the rate of a reaction related to its activation energy (Section 11-2)? Consider a bimolecular reaction that proceeds along the following pathway: where X represents the transition state. The rate of the reaction can be expressed as d[P [12-A] where k is the ordinary rate constant...
The rate of the crystal violet/NaOH reaction is given by the following generalized rate law: Rate...
The rate of the crystal violet/NaOH reaction is given by the following generalized rate law: Rate = k’[CV+]y where k’ is the pseudo rate constant defined by k’ = k [OH-]x , where k is the actual rate constant The actual rate constant can be calculated using the pseudo rate constant and the [OH-] present in the reaction mixture. If the reaction mixture is prepared by mixing 5.0 mL of 1.00 x 10-4 M crystal violet solution with 5.0 mL...
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws...
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1. You study...
#14 Rate Constant and Temperature 1. The rate constant (k) for a reaction was measured as...
#14 Rate Constant and Temperature 1. The rate constant (k) for a reaction was measured as a function of temperature. A plot of lnk versus 1/T (in K) is linear and has a slope of -1.01 x 104 K. Calculate the activation energy for this reaction. 2. The rate constant of a reaction at 32.0oC is 0.0550 s-1. If the frequency factor is 1.20 x 1013 s-1, what is the activation energy? 3. A reaction has a rate constant of...
Define the following terms: 3. Rate а. b. Rate law: Rate constant, k: c. What would...
Define the following terms: 3. Rate а. b. Rate law: Rate constant, k: c. What would you expect to happen to the rate of the reaction between iodide ion and persulfate ion (Reaction 1), as temperature increases? Explain your answer in terms of kinetic theory 4.
Method of Initial Rates Practice: You've been tasked with finding the rate constant, k, of a...
Method of Initial Rates Practice: You've been tasked with finding the rate constant, k, of a reaction that has the following rate law: rate = k [E]y [F] Under conditions where [F]>>[E] such that [F] is a constant, you measured the rate of the reaction at four different initial concentrations of [E] and calculated the initial reaction rate of each reaction. The data are given below. Trial [E] (× 10-6 M) [F] (M) Initial Rate (× 10-6 M/s) 1 10.0...
QUESTION 2 a) Explain why Net Present Value is considered technically superior to Payback and Accounting...
QUESTION 2 a) Explain why Net Present Value is considered technically superior to Payback and Accounting Rate of Returns as an investment appraisal technique even though the latter are said to be easier to understand by management. Highlight the strengths of the Net Present Value method and the weakness of the other two methods. (5 marks) b) Your company has the option to invest in projects T and R but finance is only available to invest in one of them....
Calculate the activation energy of a reaction if the rate constant at 555 K is 3.72...
Calculate the activation energy of a reaction if the rate constant at 555 K is 3.72 times 10^-5 and at 761 K it is 2.95 times 10^-3. Calculate the rate constant at 70 degree C for the reaction A + 3B rightarrow 2C given that the rate constant of the reaction is equal to 3.5 times 10^-1 M^-4 s^-1 at 95 degree C. (Ea = 142 kJ/mol)
extra credit Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated...
extra credit
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1....
Can someone please explain the
equilibrium rate constant and what it means and why it is used
here, and how it relates to the k and k prime shown above. Thank
you!
How is the rate of a reaction related to its activation energy (Section 11-2)? Consider a bimolecular reaction that proceeds along the following pathway: where X represents the transition state. The rate of the reaction can be expressed as d[P [12-A] where k is the ordinary rate constant...
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1. You study...
Define the following terms: 3. Rate а. b. Rate law: Rate constant, k: c. What would you expect to happen to the rate of the reaction between iodide ion and persulfate ion (Reaction 1), as temperature increases? Explain your answer in terms of kinetic theory 4.
QUESTION 2 a) Explain why Net Present Value is considered technically superior to Payback and Accounting Rate of Returns as an investment appraisal technique even though the latter are said to be easier to understand by management. Highlight the strengths of the Net Present Value method and the weakness of the other two methods. (5 marks) b) Your company has the option to invest in projects T and R but finance is only available to invest in one of them....
Calculate the activation energy of a reaction if the rate constant at 555 K is 3.72 times 10^-5 and at 761 K it is 2.95 times 10^-3. Calculate the rate constant at 70 degree C for the reaction A + 3B rightarrow 2C given that the rate constant of the reaction is equal to 3.5 times 10^-1 M^-4 s^-1 at 95 degree C. (Ea = 142 kJ/mol)
extra credit
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1....
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