Question

In a given experiment 4.0 moles of pure NOCl was placed in an otherwise empty 2.0 L container. Equilibrium was established given the following reaction: 2NOCl(g) 2NO(g) + Cl2(g) K = 1.6 × 10-5 Complete the following table. Use numerical values in the Initial row and values containing the variable "x" in both the Change and Equilibrium rows. Let x = the amount of Cl2 needed to reach equilibrium. Units are understood to be M and do not need to be included in your answers. NOCl NO Cl2 Initial Change Equilibrium 2.0 - 2x Determine the equilibrium concentrations of each substance in the system. [NOCl] = M [NO] = M [Cl2] = M

Answer #1

**we know that**

**concentration = moles / volume**

**so**

**intially**

**[NOCL] = 4 /2 = 2**

**now**

**consider the given reaction**

**2NOCl ---> 2N0 + cl2**

**now**

**usinng ICE table**

**at equilibrium**

**[NOCl ] = 2 - 2x**

**[N0] = 2x**

**[Cl2] = x**

**now**

**Kc = [Cl2] [N0]^2 / [NOCl]^2**

**so**

**Kc = [x] [2x]^2 / [2-2x]^2**

**Kc = 4x^3 / [2-2x]^2**

**Kc = 4x^3 / 4(1-x)^2**

**Kc = x3/ (1-x)^2**

**1.6 * 10-5 = x3 / (1-x)^2**

**solving**

**we get**

**x = 0.02478**

**so**

**at equilibrium**

**[NOCl] = 2 - 2x = 1.95044**

**[Cl2] = x = 0.02478 M**

**[NO] = 2x = 0.04956 M**

The decomposition of NOCl: 2NOCl (g) <---> Cl2 (g) + 2NO
(g) has an equilibrium constant of K=1.6*10^-5 at 35 degrees C. if
the initial concentration of NOCl is 0.500M, what is the
equilibrium concentration of NO?
A. 1.00*10^-4M
B. 2.00*10^-2M
C. 1.00*10^-2M
D. 2.3*10^-3M
When sodium is added to the reaction vessel, it scavenges the
chlorine gas in an exothermic reaction. What will the impact of
adding sodium be on the equilibrium of the decomposition of
NOCl?
A. Shifts...

1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5
. What are the equilibrium concentrations of each species if 1.0
mole of NOCl is initially placed in an empty
2.0 L flask? 2. A reaction vessel is charged with hydrogen
iodide, which partially decomposes to molecular hydrogen and
iodine: 2HI (g) H2(g) + I2(g): When the system comes to equilibrium
at 425 °C, PHI = 0.708 atm and 2 2 P P H I =...

17. The initial concentrations or pressures of reactants and
products are given for each of the following systems. Calculate the
reaction quotient and determine the direction in which each system
will proceed to reach equilibrium.
(a) 2NH3 (g) ⇌ N2 (g) + 3H2 (g) Kc = 17; [NH3] = 0.20 M, [N2] =
1.00 M, [H2] = 1.00 M
(b) 2NH3 (g) ⇌ N2 (g) + 3H2 (g) KP = 6.8 × 104 ; initial
pressures: NH3 = 3.0 atm,...

please answear each question
1)At equilibrium, ________.
a)the rates of the forward and reverse reactions are equal
b)the value of the equilibrium constant is 1
c)all chemical reactions have ceased
d)the rate constants of the forward and reverse reactions are
equal
e)the limiting reagent has been consumed
2)The equilibrium-constant expression depends on the ________ of
the reaction.
a)
stoichiometry
b)
mechanism
c)
the quantities of reactants and products initially present
d)
temperature
e)
stoichiometry and mechanism
3)Given the following reaction...

Can you please check my answers and tell me if they are
correct? thanks
8. Write the ionic equation for dissolution and the solubility
product (Ksp) expression for each of the following slightly soluble
ionic compounds:
(a) PbCl2
PbCl2(s) --> Pb2+(aq) +
2Cl-(aq)
Ksp
= [Pb2+][Cl-]2
(b) Ag2S
Ag2S(s) --> 2Ag+(aq)
+
S2-(aq) Ksp
=[Ag+]2[S2-]
(c) Sr3(PO4)2 Sr3(PO4)2(s)
--> 3Sr2+(aq) +
2PO43-(aq) Ksp
=[Sr2+]3[PO43-]2
(d) SrSO4 SrSO4(s)
--> Sr2+(aq) +
SO42-(aq) Ksp
=[Sr2+][SO42-]
14. Assuming that no equilibria other than dissolution are
involved,...

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