1/ The Following data was obtained while observing a reaction between nitric oxi
ID: 881114 • Letter: 1
Question
1/ The Following data was obtained while observing a reaction between nitric oxide and hydrogen:
F2(g) + 2CLO2(g) -----> 2FCLO2(g)
Experiment Initial(F2) Initial(CLO2) Initial rate
(mol/L) (mol/L) (mol/L*s)
1/ 0.10 0.010 1.2 x 10^-3
2/ 0.10 0.040 4.8 x 10^-3
3/ 0.20 0.010 2.4 x 10^-3
A/ write the rate law for this reaction
B/ calculate the rate constant for the reaction
C/ what is the order of this reaction
2/ consider the reaction N2(g) + 3H2(g) ----> 2NH3(g). At a particular moment during the reaction molecular hydrogen is reacting at the rate of 0.075 mole/liter*second. At what rate is ammonia (NH3) being formed? At what rate is molecular nitrogen reacting?
3/ Ethyl iodide decompose at a certain temperature in the gas phase as follows:
C2H5I(g) -----> C2H4(g) + HI(g)
A plot of in C2H5I versus time yields a straight line with a slope of -1.36x10^2 mol/L*min
A/ what is the order of this reaction
B/ write the integrated rate law for this reaction.
C/ Determine the rate constant for this reaction.
D/ Determine the half life for this reactions.
E/ Determine the concentration of ethyl iodide after 75 minutes if the initial concentration of ethyl iode was 0.25M
Explanation / Answer
1/ The Following data was obtained while observing a reaction between nitric oxide and hydrogen:
F2(g) + 2CLO2(g) -----> 2FCLO2(g)
Experiment Initial(F2) Initial(CLO2) Initial rate
(mol/L) (mol/L) (mol/L*s)
1 0.10 0.010 1.2 x 10^-3
2 0.10 0.040 4.8 x 10^-3
3 0.20 0.010 2.4 x 10^-3
Rate law for this reaction is :
Rate = k [F2]m [ClO2]n
k is rate constant, m and n are the orders with respect to F2 and ClO2
we find m and n
Rate exp 3/ Rate 1 = 2
2 = [F2]3m [ClO2]3n/ [F2]1m [ClO2]1n ( k is cancelled from both sides since the experiment is same. )
2 = (0.20/0.10)m ….(conc of ClO2 is same)
2 = 2m
Ln 2 = m ln 2
m = 1
order with respect to F2 = 1
lets find order with respect to ClO2
Rate (exp 2) / rate (exp 1) = 4
4 = (0.040/0.01)n
4 = 4n
ln 4 = n ln 4
n = 1
order with respect to ClO2 = 1
Rate law:
R = k [F2][ClO2]
We use exp 1 to calculate rate constant
1.2E-3 = k ( 0.10 ) ( 0.010)
k = 1.2
C. ) Overall order = m + n = 1+1 = 2
Question 2 )
Rate of decomposition of H2 = 0.075 mol/L.s
We know
-d[H2]/ 3 dt = d [NH3 ]/ 2 dt
(0.075 mol per L per s / 3)*2 = d [NH3 ]/ dt
d[NH3]/dt = 0.05 mol per L per s
Q. 3 . )
A.) For this reaction plot of ln [C2H5I] vs time is straight line that suggests the order of this reaction if first
B.) We write integrated rate law for first order
ln [A]t = -kt + ln [A]0
C) Rate constant
ln [A]t = -kt + ln [A]0
y m x + c
m = slope = -k
k = - slope
its slope is given
k is rate constant
k = - (-1.36E2)
= 1.36 E2 min-1
Rate constant
k = 1.36 E2 min-1
D) half life :
For first order reaction
t ½ = 0.693 / k
= 0.693 / 1.36E2
= 5.1 E-3 min
E.)
We use integrated rate law:
ln [CH3CH2I]= - 1.36 E2 min-1 * 75 min + ln [0.25]
ln [CH3CH2I] = -10201.4
lets take antilog of both side
[CH3CH2I]= 0
So there will no any ethyl iodide remains after 75 minute
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