Question

The rate law for decomposition of acetaldehyde is rate= k[acetaldehyde]2 what is the rate of the...

The rate law for decomposition of acetaldehyde is rate= k[acetaldehyde]2 what is the rate of the reaction when the [acetaldehyde]= 1.75 x 10-3 M and the rate constant is 6.73 x 10-6 M-1 . S-1

Homework Answers

Answer #1

Rate=K [acetaldehyde]2                  where K= 6.73 x 10-6 M-1. S-1 and [acetaldehyde]=1.75 x 10-3 M

       = 6.73 x 10-6 x (1.75 x 10-3)2

          = 6.73 x 10-6 x 1.75 x 10-3 x 1.75 x 10-3

        = 20.61 x 10-12 M. S-1

         

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The rate constant for the decomposition of acetaldehyde, CH3CHO, to methane, CH4, and carbon monoxide, CO,...
The rate constant for the decomposition of acetaldehyde, CH3CHO, to methane, CH4, and carbon monoxide, CO, in the gas phase is 1.1 × 10−2 L/mol/s at 703 K and 4.95 L/mol/s at 865 K. Determine the activation energy for this decomposition.
3)The thermal decomposition of acetaldehyde is a second order reaction CH3CHO-> CH4+CO from the data shown...
3)The thermal decomposition of acetaldehyde is a second order reaction CH3CHO-> CH4+CO from the data shown below, calculate the average rate of change in the pressure of acetaldehyde between 42 and 105 s. include the correct sign and units. ( this is analogous to finding the average rate of change in concentration, just substitute pressure for concentration.) 4) for the reaction shown below which one of the following statements can you rightly assume? 2H2S (g) +O2 (g) ->2S (s)+ 2H2O...
The thermal decomposition of acetaldehyde, CH3CHO --> CH4 + CO, is a second-order reaction. The rate...
The thermal decomposition of acetaldehyde, CH3CHO --> CH4 + CO, is a second-order reaction. The rate constant is 1.55x10-4 M-1s-1 at 25oC. If the initial concentration of CH3CHO is 0.250M. What will the concentration be after 2.50 hours?
The following data are obtained for the gas phase decomposition of acetaldehyde: k (L/mole s)    0.0105            ...
The following data are obtained for the gas phase decomposition of acetaldehyde: k (L/mole s)    0.0105             0.101               0.60                 2.92             T (K)               700                  750                  800                  850          Plot these data (ln k versus 1/T) and find the activation energy for the reaction. Please show work and graph.
The decomposition of HI (g) into its elements in the gas phase at 800 K is...
The decomposition of HI (g) into its elements in the gas phase at 800 K is found to proceed by a second order process. A) Please write a balanced equation for the reaction (smallest integer ratio of coefficients, please). B) Please write the rate law for the reaction: C) Given that it takes 142 s for the [HI (g)] to change from 6.75 x 10-2 M to 3.50 x 10-2 M, please calculate the value of the rate constant (and...
At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k =...
At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k = 2.2 x 10^5 M^-1sec^-1 H2(g) + Ar(g) → 2 H(g) + Ar(g) a. Calculate the rate of reaction when [H2] = 1.0 x 10^-3 M and [Ar] = 7.2x 10^-4 M. b. Derive an expression for t½ for a second order reaction (Rate = k[A]^2).
1) The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)  2 NO2(g) + ½ O2(g)...
1) The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)  2 NO2(g) + ½ O2(g) is first order in N2O5 with a rate constant of 4.70×10-3 s-1. If the initial concentration of N2O5 is 0.105 M, the concentration of N2O5 will be  Mafter 391 s have passed. 2) The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)2 NO2(g) + ½ O2(g) is first order in N2O5 with a rate constant of 4.70×10-3 s-1. If the initial concentration of...
The rate constant for the first-order decomposition of a compound A in the reaction 2 A...
The rate constant for the first-order decomposition of a compound A in the reaction 2 A  P is k, =3.56 x 10-7 s-1 at 25°C. What is the half-life of A? What will be the pressure, initially 33.0 kPa at (a) 50 s, (b) 20 min, (c) 20 h after initiation of the reaction?
Values of the rate constant for the decomposition of N2O5 at four different temperatures are as...
Values of the rate constant for the decomposition of N2O5 at four different temperatures are as follows: T(K) k(s^-1) 658 2.14 x 10^5 673 3.23 x 10^5 688 4.81 x 10^5 703 7.03 x 10^5 Determine the activation energy of the decomposition reaction: _____kJ/mol Calculate the value of the rate constant at 300 K. _____s^-1
What are the units of k for the rate law: Rate = k[A]2[B]2, when the concentration...
What are the units of k for the rate law: Rate = k[A]2[B]2, when the concentration unit is mol/L? A. s-1 B. L mol-1 s-1 C. L2 mol-2 s-1 D. L3 mol-3 s-1 A reaction has the following stoichiometry: H2 + 2 ICl ---> I2 + 2 HCl Which of the following would be a correct definition of the rate? A. Rate = +Δ[H2]/Δt B. Rate = +Δ[HCl]/Δt C. Rate = -Δ[ICl]/Δt D. Rate = +(1/2)Δ[HCl]/Δt
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT