The reaction 4 A + C + H ? D has the mechanism below. What is...
The reaction 4 A + C + H ? D has the mechanism below. What is
the rate law? PLEASE EXPLAIN HOW
1) 2 A ? B fast
2) 2 B ? B2 fast
3) B2 + C ? G slow
4) G + H ? D fast
What is the reaction scheme and mechanism for the halogen
exchange reaction, via an Sn2 mechanism, using benzyl bromide as
the electrophilic substrate? In this reaction, the alkyl halide
will react with sodium iodine in acetone.
The reaction, 2A + 2B → C + D, has a rate constant of 6.0 × 10-3
M-2 s-1 at 0°C. From this information, can we determine the order
of this rate law? If so what is the order?
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
0.2
0.4
2 x 10-3
2
0.2
0.2
0.4
4 x 10-3
3
0.3
0.4
0.4
6 x 10-3
4
0.4
0.6
0.2
2 x 10-3
Calculate the value of k to 3 significant figures.
Let G = Z4 × Z4, H = ⟨([2]4, [3]4)⟩.
(a) Find a,b,c,d∈G so that G is the disjoint union of the 4
cosets a+H,b+
H, c + H, d + H. List the elements of each coset.
(b) Is G/H cyclic?
What is meant by chemical equilibrium? Given the
following reaction: A + B <--> C +D (reversible
reaction), how would you drive the following reaction away
from equilibrium to produce more of substances A and
B?
For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate
was measured for various initial concentrations of reactants. The
following data were collected:
Trial
[A][A]
(MM)
[B][B]
(MM)
[C][C]
(MM)
Initial rate
(M/sM/s)
1
0.30
0.30
0.30
9.0×10−5
2
0.30
0.30
0.90
2.7×10−4
3
0.60
0.30
0.30
3.6×10−4
4
0.60
0.60
0.30
3.6×10−4
Rate law equation
The rate of a chemical reaction depends on the concentrations of
the reactants. For the general reaction between AA and BB,
aA+bB⇌cC+dDaA+bB⇌cC+dD
The dependence of the...
Based on the below data what is the regression equation? a) 4 +
33X b) 33 * -1X c) -1 + 4X d) -1X + 4Regression StatisticsMultiple RR SquareAdjusted R SquareStandard ErrorObservations8ANOVAdfSSMSFRegression1333333Residual6111Total7CoefficientsStandard Errort StatP-valueIntercept-131.2746663.9842840.007248Advertising (thousands of $)46.193306741.6108020.158349
The reversible chemical reaction
A+B⇌C+D
has the following equilibrium constant:
Kc=[C][D][A][B]=3.4
Initially, only A and B are present, each at 2.00 M.
What is the final concentration of A once equilibrium is
reached?
What is the final concentration of D at equilibrium if the
initial concentrations are [A] = 1.00 M and [B] = 2.00
M ?