Consider the following equilibrium:
2NOCl(g) 2NO(g)
+ Cl2(g)with K = 1.6 × 10–5. 1.00 mole of pure...
Consider the following equilibrium:
2NOCl(g) 2NO(g)
+ Cl2(g)with K = 1.6 × 10–5. 1.00 mole of pure NOCl and 1.50 mole
of pure Cl2 are placed in a 1.00-L container. Calculate the
equilibrium concentration of NO(g).
At 35oC, K = 1.6 x 10-5 for the following
reaction
2NOCl(g) <----> 2NO(g) +
Cl2(g)
Calculate the concentration of all species at equilibrium for
each of the following original mixtures.
1) 3.0 moles of pure NOCl in a 2.0 L flask
2) 2.0 moles of NOCl and 2 moles of NO in a 3 L flask
3) 3.0 moles of NOCl 1 mole of Cl2 in a 2.0 L
flask
Show work please
The reaction 2NO(g) + Cl2(g) --> 2NOCl(g) obeys
the rate law rate = k [NO]2 [Cl2]. The
following mechanism is proposed:
NO (g) + Cl2 (g) --> NOCl2(g)
NOCl2(g) + NO (g) -->2NOCl (g)
a) What would the rate law be if the first step was rate
determining?
b) Based on the observed rate law, what can be concluded about
the relative rates of the 2 reactions?
Q1)
part A:
Consider the decomposition of NOCl: 2NOCl(g) → 2NO(g) +
Cl2(g)
During the decomposition, the concentration of cyclopropane is
measured. By graphing [NOCl] vs. time, ln[NOCl] vs. time and
1/[NOCl] vs. time, the plot of 1/[NOCl] vs. time gives a straight
line with a slope of 9.98 x 10-2 at 129oC.
(a) What is the reaction order for the decomposition of
NOCl.
(b) Calculate the rate constant of the reaction.
(c) If the initial concentration of NOCl(g) is...
For the reaction 2NO(g) + Cl2(g) --->2NOCl(g) if the
concentration of NO is tripled, the rate of the reaction increases
by a factor of nine. if the concentration of Cl2 is cut in half,
the rate of the reaction is decreased to half the original rate.
Find the order of reaction for each reactant and write the rate
expression for the reaction.
At 35 degrees C, Kc = 1.6x10^-5 for the reaction:
2NOCl(g),<--> 2NO(g) + Cl2(g)
Calculate the concentrations of all species at equilibrium for
each of the following origional mixtures.
a. 1.00 mol NOCl in a 1.0 L container
b. 1.00 mol NO and 0.50 mol Cl2 in a 1.0 L container
c. 1.00 mol NO and 0.75 mol Cl2 in a 1.0 L container
The answers are: a. [NOCl]= 1.0M, [NO]= 0.032M, [Cl2]= 0.016M;
b. [NOCl]= 1.0M, [NO]= 0.032M, [Cl2]=...
If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g) A scientist places four moles of nitrogen monoxide and two moles of chlorine gas into flask A and the same amounts into Flask B, then allows the systems to reach equilibrium. Flask A is at 25 degrees Celsius and Flask B is at 200 degrees Celsius
A) In which flask will the reaction occur faster? Explain.
B) In which flask will the reaction occur to a greater...
Question 11 5 pts
Nitrosyl chloride, NOCl, decomposes to NO and Cl2.
2NOCl (g) ----> 2NO (g) + Cl2 (g)
Determine the overall order and rate constant "k" for this
reaction from the following data:
[NOCl] (M)
0.10
0.20
0.30
Rate (M/h)
8.0 x 10–10
3.2 x 10–9
7.2 x 10–9
The reaction
2NOCl(g)=2NO(g)+Cl2(g)
comes to equilibrium at 1 bar total pressure and 227C when the
partial pressure of the nitrosyl chloride, NOCl, is 0.64 bar. Only
NOCl was present initially. (a) Calculate
deltarGo for this reaction. (b) At what total
pressure will the partial pressure of Cl2 be at 0.1
bar?
For the following systems at equilibrium
A:2NOCl(g)⇌2NO(g)+Cl2(g) B: H2(g)+I2(g)⇌2HI(g) classify these
changes by their effect.
Drag the appropriate items to their respective bins.
Bins: leftward shift, no shift, rightward shift
Items: system A Decrease container size, system A Increase
container size, system b Increase container size, system B Decrease
container size
Consider the equilibrium between SbCl5, SbCl3 and Cl2.
SbCl5(g)<--------> SbCl3(g) + Cl2(g) K = 2.36×10-2 at 552
K
The reaction is allowed to reach equilibrium in a 6.80-L flask.
At equilibrium, [SbCl5] = 0.359 M, [SbCl3] = 9.20×10-2 M and [Cl2]
= 9.20×10-2 M.
(a) The equilibrium mixture is transferred to a 13.6-L flask. In
which direction will the reaction proceed to reach equilibrium?
(b) Calculate the new equilibrium concentrations that result
when the equilibrium mixture is transferred to a...