![N204(g) <_> 2NO2(g) (1) [NO2)^2/[N204]=Kf/Kr=a constant (2) If the rate constant for the forward reaction in Equation (1) is](http://img.homeworklib.com/questions/c899a160-d512-11eb-b86d-11c445b4de5f.png?x-oss-process=image/resize,w_560)
Homework Answers
Since equilibrium constant is defined as the rate constant of forward reaction divided by rate constant of backward reaction. If the rate constant of forward reaction is greater in comparison to rate constant of backward reaction, so equilibrium constant will be greater than 1 . C option is correct option.
Add Answer to:
N204(g) <_> 2NO2(g) (1) [NO2)^2/[N204]=Kf/Kr=a constant (2) If the rate constant for the forward reaction in...
How does the value of Kc in Equation the reaction below depend on the starting concentrations...
How does the value of Kc in Equation the reaction below depend on the starting concentrations of NO2 and N204? N204_<_> 2NO2(g) Kc- [NO2]^2/[N204] Kc is independent of the starting concentrations of reactants and products O b. Kc is independent of the starting concentrations of reactants and products. Oc. Kc is second order with respect to NO2 and inversely related to N204 using starting concentrations ke is directly related to NO2 and inversely related to N204 using starting concentrations
2. For the equilibrium between dinitrogen tetroxide and nitrogen dioxide: N204 = 2 NO2 Suppose that...
2. For the equilibrium between dinitrogen tetroxide and nitrogen dioxide: N204 = 2 NO2 Suppose that both the forward and reverse reactions are elementary processes with rate constants of k, and kr respectively, and the equilibrium constant for the process is 14.48 at 298 K. If the rate of the reverse reaction is 1324 M/s when (NO2) = 0.60 M, what is the half-life for the decomposition of dinitrogen tetroxide (the forward reaction) at the same temperature?
Consider the dimerization 2A S A2, with forward rate constant kf and reverse rate constant kr. (a) Derive an expression...
Consider the dimerization 2A S A2, with forward rate constant kf and reverse rate constant kr. (a) Derive an expression for "in terms of the rate constants, [A], and the total concentration of dt protein, [A]o[A]+2[A2] (b) The equation you derived above can be used to show that k8kk,[A]cot T2 where T is a quantity with units of time that depends the data provided below, calculate the rate constants formation of hydrogen-bonded dimers of 2-pyridone: on k, ki, and [A]ot....
10. The equilibrium constant for the reaction N204(8) = 2NO2(g) at 25 °C is 5.88 x...
10. The equilibrium constant for the reaction N204(8) = 2NO2(g) at 25 °C is 5.88 x 10-3. Suppose 15.6 g of N204(g) is placed in a 5.000-L flask at 25 °C. Calculate the following: (a) The moles of NO2(g) present at equilibrium (b) The percent dissociation of the original N,O4(g).
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
For a different reaction, Kc = 1.03, kf=86.5s−1, and kr= 83.8 s−1 . Adding a catalyst...
For a different reaction, Kc = 1.03, kf=86.5s−1, and kr= 83.8 s−1 . Adding a catalyst increases the forward rate constant to 1.47×103 s−1 . What is the new value of the reverse reaction constant, kr, after adding catalyst?
2. For the isomerization reaction, N204(g) + 2NO2(g), the degree of dissociation (a) is 0.201 at...
2. For the isomerization reaction, N204(g) + 2NO2(g), the degree of dissociation (a) is 0.201 at equilibrium (25°C and 1 bar). (NOTE: DO NOT simply look up the thermodynamic table for this question. You MUST compute all the quantities using known formula.) (a) Calculate A,G,A,Gº and K at equilibrium. (b) If the equilibrium constant at 100°C is 17.46, is this reaction exothermic or endothermic? (c) Calculate the standard reaction entropy, A. Sº, of this reaction.
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g)...
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + )...
Step 1: NO(g) + O2(g) ---> NO2(g) + O(g) rate= k1 Step 2: NO(g) + ) --> NO2 (g) rate = k2 suppose that k1<<k2, That is the first step is much slower than the second. Write the balanced chem equation for the overall chemical rxn Write the experimentally observable rate law for the overall reaction. (no reaction concentrations) rate=k() Express the rate constant k for the overall reaction in terms of k1, k2 and (if necessary) the rate constant...
Which statement concerning the reversible reaction 2 NO2(g) N2O4(g) is true? a. NO2 is the product of the...
Which statement concerning the reversible reaction 2 NO2(g) N2O4(g) is true? a. NO2 is the product of the forward reaction. b. The reverse reaction produces N2O4. c. At the start of the reaction, the forward and reverse reaction rates are equal. d. As the forward reaction progresses and more N2O4 is formed, the reverse reaction rate increases.
How does the value of Kc in Equation the reaction below depend on the starting concentrations of NO2 and N204? N204_<_> 2NO2(g) Kc- [NO2]^2/[N204] Kc is independent of the starting concentrations of reactants and products O b. Kc is independent of the starting concentrations of reactants and products. Oc. Kc is second order with respect to NO2 and inversely related to N204 using starting concentrations ke is directly related to NO2 and inversely related to N204 using starting concentrations
2. For the equilibrium between dinitrogen tetroxide and nitrogen dioxide: N204 = 2 NO2 Suppose that both the forward and reverse reactions are elementary processes with rate constants of k, and kr respectively, and the equilibrium constant for the process is 14.48 at 298 K. If the rate of the reverse reaction is 1324 M/s when (NO2) = 0.60 M, what is the half-life for the decomposition of dinitrogen tetroxide (the forward reaction) at the same temperature?
Consider the dimerization 2A S A2, with forward rate constant kf and reverse rate constant kr. (a) Derive an expression for "in terms of the rate constants, [A], and the total concentration of dt protein, [A]o[A]+2[A2] (b) The equation you derived above can be used to show that k8kk,[A]cot T2 where T is a quantity with units of time that depends the data provided below, calculate the rate constants formation of hydrogen-bonded dimers of 2-pyridone: on k, ki, and [A]ot....
10. The equilibrium constant for the reaction N204(8) = 2NO2(g) at 25 °C is 5.88 x 10-3. Suppose 15.6 g of N204(g) is placed in a 5.000-L flask at 25 °C. Calculate the following: (a) The moles of NO2(g) present at equilibrium (b) The percent dissociation of the original N,O4(g).
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
2. For the isomerization reaction, N204(g) + 2NO2(g), the degree of dissociation (a) is 0.201 at equilibrium (25°C and 1 bar). (NOTE: DO NOT simply look up the thermodynamic table for this question. You MUST compute all the quantities using known formula.) (a) Calculate A,G,A,Gº and K at equilibrium. (b) If the equilibrium constant at 100°C is 17.46, is this reaction exothermic or endothermic? (c) Calculate the standard reaction entropy, A. Sº, of this reaction.
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
Most questions answered within 3 hours.
-
1. What is the meaning of the term communication style?
2. What are the benefits to...
asked 45 seconds from now -
9.) You are buying a car that cost $26,500. You make payments of
$412 each month...
asked 24 minutes ago -
. Suppose a discrete random variable has probability
distribution
P(x) = .2 if x = 0...
asked 1 hour ago -
Problem #1
The area between Z = 0 and Z = 2.50
The area between Z...
asked 40 minutes ago -
Under the influence of its drive force, a snowmobile is moving
at a constant velocity along...
asked 2 hours ago -
Why do organizations decline? What steps can top
management take to halt, decline, and restore organizational...
asked 1 hour ago -
What mechanisms Drive speciation??
(I.e. what was Dawins theory on the orgin of species, and how...
asked 3 hours ago -
The manager at a car assembly plant believes that the mean
assembly time for a car...
asked 4 hours ago -
Which of the following is true of electron capture?
A) It decreases the nuclide's mass number...
asked 5 hours ago -
Assuming an efficiency of 43.10%, calculate the actual yield of
magnesium nitrate formed from 114.9 g...
asked 6 hours ago -
The highly pathogenic bacterium Clostridium
perfringens causes gangrene, a disease that results in the
destruction of...
asked 8 hours ago -
In the context of situation analysis, which of the following is
a category for analysis in...
asked 8 hours ago