Expt. |
Initial [A]/ molL-1 |
Initial [B]/ molL-1 |
Initial [C]/ molL-1 |
Initial Rate/10-6 molL-1s-1 |
1 |
0.024 |
0.085 |
0.032 |
6.0 |
2 |
0.096 |
0.085 |
0.032 |
96.0 |
3 |
0.024 |
0.034 |
0.080 |
15.0 |
4 |
0.012 |
0.170 |
0.032 |
1.5 |
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Expt. Initial [A]/ molL-1 Initial [B]/ molL-1 Initial [C]/ molL-1 Initial Rate/10-6 molL-1s-1 1 0.024 0.085...
Day Sample (n) Number (np) Proportion (p) 1 500 12 0.024 2 500 15 0.030 3 500 19 0.038 4 500 13 0.026 5 500 9 0.018 6 500 26 0.052 7 500 18 0.036 8 500 14 0.028 9 500 17 0.034 10 500 18 0.036 11 500 16 0.032 12 500 24 0.048 13 500 11 0.022 14 500 31 0.062 15 500 16 0.032 16 500 10 0.020 17 500 16 0.032 18 500 17 0.034 19...
A first-order reaction A⟶BA⟶B has the rate constant k=k= 2.8×10−3 s−1s−1 . If the initial concentration of AA is 1.5×10−2 MM, what is the rate of the reaction at t=t= 690 ss ? Express your answer to two significant figures and include the appropriate units.
Select the rate law that corresponds to the data shown for the following reaction. A+B Products Experiment [A] (mol dm3) 0.012 0.024 0.024 0.012 [B] (mol dm3) 0.035 0.070 0.035 2 3 4 Initial Rate(mol dm-3 3-1) 0.10 0.80 0.10 0.80 Rate = k[B] Rate = K[B] Rate = k [A] [B]3 Rate = k[A] [B]
Use the data in the table below to determine the rate constant (in L mol-1s-1) for the reaction below? 2?2(?)+?2(?)⇌2?2?(?) 2 H 2 ( g ) + O 2 ( g ) ⇌ 2 H 2 O ( g ) Experiment [H2]0 (M) [O2]0 (M) Initial rate (M s-1) 1 2.5 x 10-2 1.0 x 10-2 4 2 5.0 x 10-2 1.0 x 10-2 8 3 2.5 x 10-2 0.5 x 10-2 2 Select one: a. 1.2 x 103 3...
The rate constant for a certain reaction is kk = 7.20×10−3 s−1s−1 . If the initial reactant concentration was 0.900 MM, what will the concentration be after 7.00 minutes?
a. Given these data for the reaction A + B → C, write the rate-law expression. Use k for the rate constant.) b. What is the value, with units, for the specific rate constant? The specific rate constant- Initial Rate of Initial [A] Initial [B] Formation of C Expt. (M) (M.s-1) 0.30 0.30 0.60 0.20 0.40 0.80 4.0 x 10-5 1.6 x 10-4 2.6 x 10-3
Experiment Initial [A] Initial [B] Initial [C] Initial Rate of Reaction 1 0.1 M 0.1 M 0.2 M 4 x 10^(-4) M/min 2 0.3 M 0.2 M 0.2 M 1.2 x 10^(-3) M/min 3 0.1 M 0.3 M 0.2 M 4 x 10^(-4) M/min 4 0.3 M 0.4 M 0.6 M 3.6 x 10^(-3) The method of initial rates is used to determine the rate law for reactants A, B, and C. This data was obtained at 25 degrees C....
Products yielded the following data: 6. A reaction A+B+C Initial concentration (mmol L-1) Initial rate (-d[Al/dt) (mmol L-1 s-1) Experiment AI) 0 [C]O Initial rate (-dA/dt mM I-S-1) [BJO 8.72 11.25 1.25 1.25 2.50 1.25 1.25 17.4 3 1.25 3.02 1,25 50.84 3.75 457 1.25 3.02 a) Write the rate law for this reaction b) If the initial reactant concentrations were [A]0 2 mmol L-1, [Bl0 1.5 mmol L-1 and [C]0 =1.15 mmol L-1, indicate what would be the initial...
4. For the reaction 2A+B → CD+E Experiment [B] 0.015 0.006 0.015 0.012 0.045 0.012 Initial Rate, M/min 0.0195 0.039 0.120 2C 5. For the reaction 2A +B Experiment 1 8.0x102 4 .0x102 3 8.0x102 1 [B] 2.0x102 1.0x102 4.0x102 Initial Rate, M/min 4.0x10 1.0x10 4.0x10 2 76. Use the following data for the reaction: 4CH N O the rate when [CH.N) is 0.004 M and [O] is 0.02 M → CO+H,0 + 4NO. Find Experiment 2 CHEN 3.8 x...
1. Initial rate data at 25.0 °C are listed below for the reaction: 2 HgCl2 (aq) C2O (aq)2 C (aq)+ 2 CO:(g)+ Hg Cl(s) (COP)0 Expt. HgClalo Initial rate/ 3.1 x 10 1 0.100 0.20 1.2x 10 0.100 0.40 6.2x 10S 0.050 0.40 Use the data to determine the rate law for the reaction. 2. At 500 °C, cyclopropane (CsH6) rearranges to propene (CH3CH-CH2): CH CH=CH2 (g) CaHs (g) The reaction is first order and the rate constant is 6.7...