Question
In: Chemistry
1. The densities of crystalline Cl2 and H2S at 160 K are 2.02 and 0.95 g/cm3,...
1. The densities of crystalline Cl2 and H2S at 160 K are 2.02 and 0.95 g/cm3, respectively. Calculate their molar volumes.
2. The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol.
Calculate the heat required to convert 73.0 g of C2Cl3F3 from a liquid at 13.90 ∘C to a gas at 99.80 ∘C.
Express your answer using two significant figures.
Solutions
queen_honey_blossom answered 4 weeks agoRelated Solutions
1) The equilibrium constant, K, for the following reaction is 2.02×10-2 at 513 K. PCl5(g) <------...
1) The equilibrium constant, K, for the following reaction is
2.02×10-2 at 513 K. PCl5(g) <------ ------> PCl3(g) + Cl2(g)
An equilibrium mixture of the three gases in a 18.3 L container at
513 K contains 0.216 M PCl5, 6.60×10-2 M PCl3 and 6.60×10-2 M Cl2.
What will be the concentrations of the three gases once equilibrium
has been reestablished, if the equilibrium mixture is compressed at
constant temperature to a volume of 8.25 L?
[PCl5] = ______M
[PCl3] =...
1) For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g)...
1) For the following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) ⇌ COCl2 (g)
A reaction mixture initially contains a COconcentration of 0.1550 M
and a Cl2concentration of 0.175 M at 1000 K.
1a)What is the equilibrium concentration of
CO at 1000 K?
1b)What is the equilibrium concentration of
Cl2 at 1000 K?
c)What is the equilibrium concentration of
COCl2 at 1000 K?
2) At 650 K, the reaction MgCO3(s)⇌MgO(s)+CO2(g) has Kp=0.026. A
12.5 L...
The reaction 2NO(g) + Cl2(g) --> 2NOCl(g) obeys the rate law rate = k [NO]2 [Cl2]....
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?
1) At a certain temperature, 322 K, Kp for the reaction, Cl2(g) <=> 2 Cl(g), is...
1) At a certain temperature, 322 K, Kp for the
reaction,
Cl2(g) <=> 2 Cl(g), is 7.82 x
10-60.
Calculate the value of ΔGo in kJ for the reaction at
this temperature.
2)
The equilibrium constant for the reaction,
2 Fe3+(aq) + Hg22+(aq)
<=> 2 Fe2+(aq) + 2 Hg2+(aq)
is 9.1 x 10-6(aq) at 298 K. Calculate ΔG in J when
{Fe3+(aq)} = 0.375
{Hg22+(aq)} = 0.051
{Fe2+(aq)} = 0.021
{Hg2+(aq)} = 0.06
1. A student ran the following reaction in the laboratory at 582 K: CO(g) + Cl2(g)...
1. A student ran the following reaction in the laboratory at
582 K:
CO(g) + Cl2(g)
COCl2(g)
When she introduced 0.380 moles of
CO(g) and 0.403 moles of
Cl2(g) into a 1.00 liter container, she
found the equilibrium concentration of
COCl2(g) to be 0.342
M.
Calculate the equilibrium constant, Kc, she obtained for
this reaction.
2. The equilibrium constant, Kc, for the following
reaction is 1.29×10-3 at
540 K.
COCl2(g) CO(g) +
Cl2(g)
When a sufficiently large sample of
COCl2(g)...
1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K calculate the equilibrium...
1.For the reaction,
PCl5(g) <-----> PCl3(g) +
Cl2(g) Kp
= 24.6 at 500 K
calculate the equilibrium partial pressures of the reactants and
products if the initial pressures are PPCl5 =
0.610 atm, PPCl3 = 0.400 atm and
PCl2 = 0.000 atm.
PPCl5 = PPCl3 =
PCl2 =
2.
H2O(g) + Cl2O(g) <----->
2HClO(g) Kc
= 0.14 at 298.15 K
calculate the equilibrium concentrations of the reactants and
products if the initial concentrations are [H2O(g)] =
0.00482 mol L-1, [Cl2O(g)] = 0.00482...
Consider the equilibrium between SbCl5, SbCl3 and Cl2. SbCl5(g)<--------> SbCl3(g) + Cl2(g) K = 2.36×10-2 at...
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...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) ⇌ COCl2 (g)
A reaction mixture initially contains a COconcentration of 0.1510
M and a Cl2concentration of 0.179 M at 1000
K.
What is the equilibrium concentration of CO at 1000 K?
What is the equilibrium concentration of Cl2 at 1000 K?
What is the equilibrium concentration of COCl2 at 1000 K?
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the
following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) ⇌ COCl2 (g)
You may want to reference (Pages 693 - 702)Section 15.8 while
completing this problem.
Part A
If a reaction mixture initially contains a CO concentration of
0.1550 and a Cl2 concentration of 0.175 at 1000K. What is the
equilibrium concentration of CO at 1000 K?
Express your answer in molarity to three significant
figures.
[CO]=
nothing
M
SubmitRequest Answer
Part B
What...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) ⇌ COCl2 (g)
A reaction mixture initially contains a COconcentration of 0.1470
M and a Cl2concentration of 0.179 M at 1000
K.
Part a. What is the equilibrium concentration of CO at 1000
K?
Part B:What is the equilibrium concentration of Cl2 at 1000
K?
Part C:What is the equilibrium concentration of COCl2 at 1000
K?
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