Question

The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH4NCO(aq)(NH2)2CO(aq) is second...

The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH4NCO(aq)(NH2)2CO(aq) is second order in NH4NCO. In one experiment, when the initial concentration of NH4NCO was 0.416 M, the concentration of NH4NCO dropped to 6.49×10-2 M after 828 minutes had passed. Based on these data, the rate constant for the reaction is ______M-1 min-1.

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
Ammonium cyanate, NH4NCO, rearranges in water to give us urea., (NH2)2 CO: NH4NCO (AQ) to ((NH2))2CO...
Ammonium cyanate, NH4NCO, rearranges in water to give us urea., (NH2)2 CO: NH4NCO (AQ) to ((NH2))2CO (AQ). The rate for this equation for the process is "rate =k (NH4NCO)2," where k =0.113 L/mol per min. If the original concentration in the solution is 0.229mol/L, how long will it take for the concentration to decrease to 0.180 mol/L?
1. The pH of an aqueous solution of 0.285 M ammonium iodide, NH4I (aq), is _____....
1. The pH of an aqueous solution of 0.285 M ammonium iodide, NH4I (aq), is _____. This solution is (acidic, basic, neutral)
The reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2- --->   N2...
The reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2- --->   N2 + 2 H2O is first order in NH4+ and first order in NO2-. Complete the rate law for this reaction. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to...
1) What is the pH of a 0.100 M NH4Cl(aq) solution? 2) The reaction A(aq) +...
1) What is the pH of a 0.100 M NH4Cl(aq) solution? 2) The reaction A(aq) + B(aq) → 2C(aq) has an equilibrium constant of Kc= 5.2. If the initial concentrations are [A] = 0.100 M, [B] = 0.000 M, and [C] = 0.500 M, what are the concentrations of A, B, and C at equilibrium? 3) What are the concentrations of H3O+, H3PO4, H2PO4-, and HPO42- in a 0.100 M H3PO4(aq) solution? (In this solution, 0.100 M would be the...
The decomposition reaction of NOBr is second order in NOBr, with a rate constant at 20°C...
The decomposition reaction of NOBr is second order in NOBr, with a rate constant at 20°C of 25 M-1 min-1. If the initial concentration of NOBr is 0.025 M, find (a) the time at which the concentration will be 0.010 M. (b) the concentration after 145 min of reaction.
1) The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½...
1) The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3 min-1. If the initial concentration of H2O2 is 9.20×10-2 M, the concentration of H2O2 will be 1.83×10-2 M after____________ min have passed. 2) The gas phase decomposition of dimethyl ether at 500 °C CH3OCH3(g) CH4(g) + H2(g) + CO(g) is first order in CH3OCH3 with a rate constant of 4.00×10-4 s-1. If...
1.) 2A → B + C The above reaction is run and found to follow second...
1.) 2A → B + C The above reaction is run and found to follow second order kinetics with a rate constant of 1.30 x 10-3 M-1sec-1. If the initial concentration of A is 1.33 M, what is the concentration after 164 seconds? 2.) 2A → B + C Two trials of the above reaction are run with the same initial concentration of A. The first trial is performed at 25oC and the second at 35oC. If the rate constant...
1.) Consider the reaction of peroxydisulfate ion (S2O2−8) with iodide ion (I−) in aqueous solution: S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−3(aq)....
1.) Consider the reaction of peroxydisulfate ion (S2O2−8) with iodide ion (I−) in aqueous solution: S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−3(aq). What is the rate of disappearance of I− when [S2O2−8]= 3.5×10−2 M and [I−]= 5.5×10−2 M ? 2.) Consider the reaction 2H3PO4→P2O5+3H2O Using the information in the following table, calculate the average rate of formation of P2O5 between 10.0 and 40.0 s. Time (s)010.0, 20.0, 30.0, 40.0, 50.0[P2O5] (M)02.20×10−3, 5.20×10−3, 7.00×10−3, 8.20×10−3, 8.80×10−3 3.) The reactant concentration in a second-order reaction was 0.470 M...
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...
Consider the reaction of peroxydisulfate ion (S2O2−8S2O82−) with iodide ion (I−I−) in aqueous solution: S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−3(aq)S2O82−(aq)+3I−(aq)→2SO42−(aq)+I3−(aq). At...
Consider the reaction of peroxydisulfate ion (S2O2−8S2O82−) with iodide ion (I−I−) in aqueous solution: S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−3(aq)S2O82−(aq)+3I−(aq)→2SO42−(aq)+I3−(aq). At a particular temperature the rate of disappearance of S2O2−8S2O82− varies with reactant concentrations in the following manner: Experiment S2O2−8(M)S2O82−(M) I−(M)I−(M) Initial Rate (M/s)(M/s) 1 0.018 0.036 2.6×10−62.6×10−6 2 0.027 0.036 3.9×10−63.9×10−6 3 0.036 0.054 7.8×10−67.8×10−6 4 0.050 0.072 1.4×10−5 What is the average value of the rate constant for the disappearance of S2O2−8S2O82− based on the four sets of data? How is the rate...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT