Question

1) Initial concentration of reactant A in a 2nd-order reaction aA ----> Products is 0.880 M....

1) Initial concentration of reactant A in a 2nd-order reaction aA ----> Products is 0.880 M. In 30 min, the concentration of A decreases to 40.0% of its initial value. Determine the rate constant of this reaction

2) For the reaction N2O4(g) = 2NO2(g), the equilibirum constant at definite temperature Kc = 3.5 x 10^-4. If the initial concentration of N2O4 is 0.200M, what will be the concentration of NO2 at equilibrium?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The reaction in which NO2 forms a dimer is second order in NO2 : 2NO2(g) --->...
The reaction in which NO2 forms a dimer is second order in NO2 : 2NO2(g) ---> N2O4(g) Rate = k [NO2]2 Calculate the rate constant for this reaction if it takes 0.0050 s for the initial concentration of NO2 to decrease from 0.50M to 0.25M.
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C if the initial concentrations are...
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C if the initial concentrations are [N2O4]= 0.0210 M and [NO2]= 0.0340 M. The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. 1) Calculate the equilibrium concentration of N2O4. 2) Calculate the equilibrium concentration of NO2. I have worked through this problem several times and keep getting the wrong answer. I think I'm making a math error along the way. Could you show as much work...
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C in a vessel that contains...
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C in a vessel that contains an initial N2O4 concentration of 0.0365 M . The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. Express your answers using four decimal places separated by a comma.
The reactant concentration in a zero-order reaction was 6.00×10−2 M after 160 s and 1.50×10−2 M...
The reactant concentration in a zero-order reaction was 6.00×10−2 M after 160 s and 1.50×10−2 M after 305 s . What is the rate constant for this reaction? (I got this answer 3.10*10^-4 M/s) What was the initial reactant concentration for the reaction described in Part A? The reactant concentration in a first-order reaction was 0.100 M after 40.0 s and 3.80×10−3M after 90.0 s . What is the rate constant for this reaction? (I got this answer 6.54*10^-2 1/s)...
1. Calculate hte freezing point of a 2.1 molality solution of iron(III) nitrate nonahydrate 2. Do...
1. Calculate hte freezing point of a 2.1 molality solution of iron(III) nitrate nonahydrate 2. Do trans isomers have no free-rotation? Why 3. The initial concentratio of N2O4 is 1.0M. The system is heater and allowed to reach equilibrium. At equilibirum concentration of NO2 is 0.12M. Calculate the equilibirum constant for the reaction: N2O4 <=>2NO2 4. What is an amphiprotic species? Describe why aluminum hydroxide precipitate can redissolve into solution if the pH of the solution in changed
1A. For a first order reaction, the rate will double if a.      Concentration of a reactant...
1A. For a first order reaction, the rate will double if a.      Concentration of a reactant is doubled b.     Concentration of a product is doubled c.      Concentration of a reactant is squared d.     Temperature is raised two degrees e.    2 moles of catalyst are added 1B.     For a second order decomposition reaction (one reactant), if the concentration of the reactant is tripled, the rate: a.      Triples b.     Increases nine-fold c.      Decreases by one third d.     Stays the same
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of...
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of the reactant is 0.0100M, what is the concentration remaining after 15 min? a) .0099M b) .0056M c) .0025M d) .0064M 2) the rate constant for the first order decomposition of A at 500 degrees Celsius is 9.2 x 10 to the negative 3rd powers s-1. How long will it take for 90.8 % of a 0.500M sample of A to decompose a) 2.5 x...
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C in a vessel that contains...
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C in a vessel that contains an initial N2O4 concentration of 0.0438 M . The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. Express your answers using four decimal places separated by a comma. [N2O4], [NO2] = _________________________ The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are...
A) The reaction of CH4 is carried out at a different temperature with an initial concentration...
A) The reaction of CH4 is carried out at a different temperature with an initial concentration of [CH4]= 9.1�10?2M . At equilibrium, the concentration ofH2 is 2.0�10?2M . 2CH4(g)?C2H2+3H2(g). Find the equilibrium constant at this temperature. B) The reaction between CO and H2 is carried out at a different temperature with initial concentrations of[CO] = 0.35M and [H2]= 0.60M . CO(g)+2H2(g)?CH3OH(g) At equilibrium, the concentration of CH3OH is 0.12M . Find the equilibrium constant at this temperature.
Consider the following reaction and associated equilibrium constant: aA(g)⇌bB(g), Kc = 3.8 PART A Find the...
Consider the following reaction and associated equilibrium constant: aA(g)⇌bB(g), Kc = 3.8 PART A Find the equilibrium concentrations of A and B for a=1 and b=1. Assume that the initial concentration of A is 1.0 M and that no B is present at the beginning of the reaction. PART B Find the equilibrium concentrations of A and B for a=2 and b=2. Assume that the initial concentration of A is 1.0 M and that no B is present at the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT