In the reaction A + 2B ---> 3C + D , If 93g of A and...
In the reaction A + 2B ---> 3C + D , If 93g of A and 85g of B
are combined, which reactant is the limiting reagent, and what is
the theoretical yield of C in grams? (MM(A)= 55g/mole, MM(B)=
48g/mole, MM(C)= 37g/mol)
The reaction A + 2B C + D is taking place in a batch reactor.
(Cao =1M, Cbo = 3M k=0.001 (1/M^2*min)). a) Assuming an elementary
rate law, find the time necessary to reach the conversion of 0.9.
You can assume constant volume batch reactor with well mixing. Also
form the stoichiometric table. (15 points) b) Sometimes it is hard
to obtain numerical solutions to the complex integrals. Find the
answer using trapezoidal, Simpson 1/3 and Simpson 3/8, Five-point...
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?
Using the given data, determine the rate constant of this
reaction.
A+2B ------> C+D
Trial [A](M) [B](M) Rate (M/s)
1. 0.270 0.380 0.0235
2 0.270 0.760 0.0235
3 0.540 0.380 0.0940
K=?
What units should be used?
Consider the following reaction:
2A+3B→3C+2D
Use the following data to determine the rate of reaction in
terms of the disappearance of reactant A at time = 20 s.
Time (s)
0
20
40
[A](M)
0.0400
0.0240
0.0180
Part B::Consider the following reaction:
2A+3B→3C+2D
Use the following data to determine the rate of reaction in
terms of the appearance of product C when the time is 20 s.
Time (s)
0
20
40
[C](M)
0.000
0.0240
0.0480
Part C:
Consider the...
3. Considering the reaction:
2Fe2O3 + 3C --> 4Fe + 3CO2
A. How many moles of C are needed to react with 6.00 moles of
Fe203
B. How many grams of Fe result when 175g of
Fe2O3 react?
4. Using the bond energies below determine the value and sign of
delta H for..
H-S-H + Cl-Cl --> Cl-S-Cl + H-H
Bond energies in kJ/mol:
H-S 365 Cl-Cl 240 Cl-S 255 H-H 432
5. Will a 1.0m solution of ZnCl2...
Consider the reaction
A+2B⇌CA+2B⇌C
whose rate at 25 ∘C∘C was measured using three different sets of
initial concentrations as listed in the following table:
Trial
[A][A]
(MM)
[B][B]
(MM)
Rate
(M/sM/s)
1
0.50
0.050
1.5×10−2
2
0.50
0.100
3.0×10−2
3
1.00
0.050
6.0×10−2
Part A
What is the rate law for this reaction?
Express the rate law symbolically in terms of kkk, [A][A], and
[B][B].
View Available Hint(s)
Using the given data, determine the rate constant of this
reaction.
A + 2B --> C + D
Given Data:
Trial [A](M) [B](M) RATE (M/s)
1 .230 .330 0.0231
2 .230 .660 0.0231
3 .460 .330 0.0924
k=? the units are M-1 s-1