Question
In: Chemistry
Consider two reaction vessels, one containing A and the other containing B with equal concentrations at...
Consider two reaction vessels, one containing A and the other containing B with equal concentrations at t= 0/ If both substances decompose by first order kinetics where ka =4.50e-4s^-1 kb=3.70e-3s^-1 how much time must pass to reach a condition such that [A] = 4.00[B]?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Consider the nonenzymatic elementary reaction A + B → C. When the concentrations of A and...
Consider the nonenzymatic elementary reaction A + B → C. When
the concentrations of A and B are each 25.0 mM, the reaction
velocity is measured as 4.11 µM C produced per minute.
Calculate the rate constant for this reaction with units!.
What is the molecularity of the above reaction?
If this reaction is in zero order kinetics how long would it
take to produce 2.25 x 10-3 moles of C from a starting
concentration of reactants A and B...
A reaction was run with two different initial concentrations of reactants A and B: Experiment A...
A reaction was run with two different initial concentrations of
reactants A and B:
Experiment
A / M
B / M
rateB / (M/sec)
1
0.00022
0.00046
0.0841
2
0.00022
0.00166
0.3035
What is the order of the reaction with respect to B?
A reaction was run with two different initial concentrations of
reactants A and B:
Experiment
A / M
B / M
rateB / (M/sec)
1
0.00057
0.00067
0.0000825
2
0.00057
0.00621
0.0657
What is the order of...
Consider that you are fabricating reaction vessels that are to be rated for 500 psi. The...
Consider that you are fabricating reaction vessels that are to
be rated for 500 psi. The vessels obviously have a range of
bursting pressures...but you certainly can't measure all of the
bursting pressures, because then you would have nothing to sell.
Suppose you measure the bursting pressure of a sample of the
vessels. You ask the question: is there any evidence that the
average bursting pressure of the population would be less than 500
psi? You don't want to sell...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the
equilibrium concentrations of A, B, and C for each of the following
different values of Kc. Assume that the initial concentration of A
in each case is 1.0 M and that the reaction mixture initially
contains no products. Make any appropriate simplifying
assumptions.
-------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------
Part A
Kc= 1.8
Express your answer using two significant figures. Enter your
answers numerically separated by commas.
------------------------------------------------------------------------------------------------------------------------------------------------------------------------
Part B
Kc= 1.0×10−2
Express your answer using two significant...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the
equilibrium concentrations of A, B, and C for each of the following
different values of Kc. Assume that the initial concentration of A
in each case is 1.0 M and that the reaction mixture initially
contains no products. Make any appropriate simplifying
assumptions.
Part A: Kc= 1.0 Express your answer using two
significant figures. Enter your answers numerically separated by
commas.
Part B: Kc= 2.0×10−2 Express your
answer using two significant figures. Enter...
If you mix equal concentrations of reactants and products, which of the following reaction proceed to...
If you mix equal concentrations of reactants and products, which
of the following reaction proceed to the right and which proceed to
the left?
a. H2CO3(aq) + HSO4−
(aq) ⇌ H2SO4(aq) +
HCO3− (aq)
b. HF(aq) + Cl− (aq) ⇌ HCl(aq) + F−
(aq)
c. HF(aq) + NH3(aq) ⇌ NH4 + (aq) +
F− (aq)
d. HSO4− (aq) + CN− (aq) ⇌
HCN(aq) + SO42−(aq)
e. [Al(H2O)6] 3+(aq) +
OH− (aq) ⇌
[Al(H2O)6(OH)]2+ (aq) +
H2O(l)
Part A Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will...
Part A
Calculating equilibrium concentrations when the net reaction
proceeds forward Consider mixture B, which will cause the net
reaction to proceed forward. Concentration (M) initial: change:
equilibrium: [XY] 0.500 −x 0.500−x net→ ⇌ [X] 0.100 +x 0.100+x +
[Y] 0.100 +x 0.100+x The change in concentration, x , is negative
for the reactants because they are consumed and positive for the
products because they are produced.
Based on a Kc value of 0.160 and the given data table,
what...
Part A Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will...
Part A
Calculating equilibrium concentrations when the net reaction
proceeds forward Consider mixture B, which will cause the net
reaction to proceed forward. Concentration (M) initial: change:
equilibrium: [XY] 0.500 −x 0.500−x net→ ⇌ [X] 0.100 +x 0.100+x +
[Y] 0.100 +x 0.100+x The change in concentration, x , is negative
for the reactants because they are consumed and positive for the
products because they are produced.
Based on a Kc value of 0.160 and the given data table,
what...
Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the...
Calculating equilibrium concentrations when the net reaction
proceeds forward
Consider mixture B, which will cause the net reaction to proceed
forward.
Concentration
(M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x
The change in concentration, x, is negative for the
reactants because they are consumed and positive for the products
because they are produced.
Part B
Based on a Kc value of 0.260 and the given data table,
what are the equilibrium concentrations of XY, X, and Y,
respectively?
Express the molar concentrations numerically.
[XY], [X], [Y] =
M ...
Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the...
Calculating equilibrium concentrations when the net reaction
proceeds forward
Consider mixture B, which will cause the net reaction to proceed
forward.
Concentration
(M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x
The change in concentration, x, is negative for the
reactants because they are consumed and positive for the products
because they are produced.
Part B
Based on a Kc value of 0.170 and the given data table,
what are the equilibrium concentrations of XY, X, and Y,
respectively
Calculating equilibrium concentrations when the net reaction
proceeds in reverse...
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