Use the data in the table below to determine the rate law for the following reaction . ?(?)+?(?)→?(?) A ( g ) + B ( g ) → C ( g ) Experiment [A]0 (M) [B]0 (M) [C]0 (M) Initial rate (M/s) 1 0.1 0.1 0 1 x 10-3 2 0.2 0.1 0 4 x 10-3 3 0.1 0.3 0 9 x 10-3
Select one:
a. ????=?[?][?][?] r a t e = k [ C ] [ A ] [ B ]
b. ????=?[?][?] r a t e = k [ A ] [ B ]
c. ????=?[?]2[?]2 r a t e = k [ A ] 2 [ B ] 2
d. ????=?[?]4[?]9 r a t e = k [ A ] 4 [ B ] 9
e. ????=?[?]2[?]3 r a t e = k [ A ] 2 [ B ] 3
Use the data in the table below to determine the rate law for the following reaction...
QUESTION 9 Initial rate, mol/L.s Given the data below for the reaction, 2A + 2B + 4C => D + E +3 F Experiment Initial conc of A Initial conc of B. Initial conc of C, mol/L mol/L mol/L 0.1 0.1 0.2 0.3 0.3 0.4 N 0.2 2 x 10-3 4x 10-3 6 x 103 8x10-3 w A Calculate the value of k to 3 significant figures. QUESTION 7 For the reaction, 2 A(g) + 2 B(g) => C(g) +...
Given the data below for the reaction, 2 A + 2 B + 4 C => D + E + 3 F Experiment Initial conc of A, mol/L Initial conc of B, mol/L Initial conc of C, mol/L Initial rate, mol/L.s 1 0.1 0.1 0.2 2 x 10-3 2 0.2 0.3 0.2 6 x 10-3 3 0.3 0.1 0.2 2 x 10-3 4 0.4 0.3 0.4 1.2 x 10-2 Calculate the value of k to 3 significant figures.
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....
Given the data below for the reaction, 2 A + 2 B + 4 C => D + E + 3 F, the reaction is ( ) order in A,( ) order in B, ( ) order in C and ( ) order overall. USE WORDS TO FILL IN THE BLANKS NOT NUMBERS (i.e., zero, first, second etc) !!!!! : Experiment Initial conc of A, mol/L Initial conc of B, mol/L Initial conc of C, mol/L Initial rate, mol/L.s 1...
Determine the rate law given for the following reaction given the initial rate data in the table: 2A + 2BC+2D Experiment [A] (M) [B] (M) Initial rate (M/s) 0.0211 0.113 2.00 x 10-5 2 0.0422 0.113 8.00 x 10-5 3 0.0422 0.226 1.60 x 10 1 Rate = K[A] [B] Rate = K[A] [B] Rate - AllB12 Rate - [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...
Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.033 1.84 × 10-4 0.066 7.37 × 10-4 0.099 1.66× 10-3 A. Rate = 5.6 × 10-1 M-1/2s-1[N2O5]3/2 B. Rate = 1.7 × 10-1 M-1s-1[N2O5]2 C. Rate = 1.7 × 10-1M1/2s-1[N2O5]1/2 D. Rate = 6.0 × 10-1 M-2s-1[N2O5]3 E. Rate = 5.2 × 10⁻1 s-1[N2O5]
An experiment was conducted to determine the rate law for the reaction A2(g)+B(g)→A2B(g) . The table above shows the data collected. Based on the data in the table, which statement is correct? Trial 1 [A2] 0.10 [B] 0.50 0.20 0.50 Nm + Initial rate (Ms-1) 2.5 10-4 5.0 x 10-4 5.0 x 10-5 1.0 x 10-4 0.30 0.05 1 0.30 0.10 An experiment was conducted to determine the rate law for the reaction A2(g) +B(g) → A2B(g). The table above...
From the data table determine the rate law for reactions 1-4 and calculate the value of k for each. Thanks I-IV BACKGROUND INFORMATION Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2 Concentration= 0.44 M •Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M •Calculation of I^- after mixing for parts I,II, IV= 0.10 M •Calculation of Initial (mol/L-s) Filled in Table Now the solutions for Rate Order and Rate Constant are needed Reactants 8 ml 30% HO, 2...
need help with #3 please QUESTION 3 Determine the rate-law expression for the reaction below at the temperature at which the tabulated initial rate data were obtained, rate- A + 2B + 3C - Products Experiment Initial [A] 0.10 M Initial [B] 0.20 M Initial [C] 0.10 M 0.40 M 0.20 M 0.10 M Initial Rate of Loss of A 4.0 x 10-2 Mmin 4.0 x 10-2 M/min 1.0 x 10- M'min 16x 10- Mmin 0.20 M 0.25 M 0.40...