Question

At a given temperature, K_{p} = 19 for the
reaction,

N_{2}O_{4}(g) <=> 2 NO_{2}(g)

For which system is the value of K_{p} = 361?

Please show work so I can figure out what I am doing wrong. Thank you!

Answer #1

For given transformation,

N_{2}O_{4}(g) <======> 2
NO_{2}(g)

Equilibrium constant Kp can be written as,

Kp = (P_{NO2})^{2}/(P_{N2O4})

And

Kp =19 given

So, (P_{NO2})^{2}/(P_{N2O4}) = 19

Squaring on both side we get,

[(P_{NO2})^{2}/(P_{N2O4})]^{2} =
(19)^{2}

(P_{NO2})^{4}/(P_{N2O4})^{2} =
361

(P_{NO2})^{4}/(P_{N2O4})^{2} =
Pk’

This expression indicate, the stoichiometric transformation,

2N_{2}O_{4}(g) <======= >
4NO_{2}(g)

Hence for this 2N_{2}O_{4}(g) <======= >
4NO_{2}(g) system Kp =361.

=========================================

At a particular temperature, Kp = 0.26 for the reaction below.
N2O4(g) equilibrium reaction arrow 2 NO2(g) (a) A flask containing
only N2O4 at an initial pressure of 4.9 atm is allowed to reach
equilibrium. Calculate the equilibrium partial pressures of the
gases. b) he volume of the container in part (a) is decreased to
one-half the original volume. Calculate the new equilibrium partial
pressures.

Calculate the equilibrium concentrations of N2O4 and NO2 at 25
∘C if the initial concentrations are [N2O4]= 0.0210 M and [NO2]=
0.0340 M. The equilibrium constant Kc for the reaction
N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C.
1) Calculate the equilibrium concentration of N2O4.
2) Calculate the equilibrium concentration of NO2.
I have worked through this problem several times and keep
getting the wrong answer. I think I'm making a math error along the
way. Could you show as much work...

1- Above what temperature is the following reaction
spontaneous?
N2O4(g) ↔ 2
NO2(g)
ΔH° = 57.24 kJ/mol ΔS° = 175.5 J/mol∙K
Group of answer choices
326 K
53.2 K
307 K
273 K
2- Predict the sign on ΔG for the following reaction when
PI2 = PH2 = 0.01 atm and PHI = 1.0
atm.
H2(g) + I2(g) ↔ 2
HI(g) ΔG° = -15.94 kJ/mol & Kp,298K =
620
Group of answer choices
ΔG = 0
ΔG > 0
ΔG...

9.Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) +
SO2(g) A reaction mixture initially contains 0.86 atm NO and 0.86
atm SO3. Determine the equilibrium pressure of NO2 if Kp for the
reaction at this temperature is 0.0118
please show as much detail as you can!

At 25 C, the equilibrium constant for the reaction 2A(g)
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If the three gases are mixed in a rigid container having partial
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is the system at equilibrium?
Potential answers:
The forward reaction must proceed to establish equilibrium, The
volume of the container must be known to answer the question, The
concentrations of all substances must be known to answer...

Figure out what is wrong with each questions and
answers:
1.) For the reaction 2A(g)+3B(g)⇌C(g)
Kc = 78.0 at a temperature of 239 ∘C
.Calculate the value of
Kp.
Ans: Kp=2.50 x
10^-5
2.) For the reaction
X(g)+2Y(g)⇌3Z(g)
Kp = 1.38×10−2 at a temperature of 81
∘C .Calculate the value
of Kc.
Ans: Kc = 1.38 x 10^-2
3.) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g)
K = 0.145 at 1590 ∘C . What is Kp
for the reaction at this temperature?
Ans:...

A) Calculate KP at 298 K for the reaction
NO(g)+1/2O2(g)→NO2(g) assuming that ΔH∘R is
constant over the interval 298-600K.
NOTE: I can tell you for sure the following answers are wrong:
7.2*10^10; 1.38*10^-11; 10.35; 14.65
B: Calculate KP at 475 K for this reaction
assuming that ΔH∘R is constant over the interval
298-600 K.
My prof told me to use: ln(K2/K)=-ΔH/(1/T2-1/T1) but it is not
working for me
NOTE: the following answers are wrong: 1.16*10^7; 6.26*10^6;
102

Calculate KP at 298 K for the reaction
NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is
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Calculate KP at 496 K for this reaction
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Do you expect KP to increase or decrease as
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2NO2(g)↔N2O4(g) if the
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the reaction favor product or reactant at this temperature?
14-2) For the reaction shown, Kc= 5.88 X 10-32
Ag2S(s)
+2H+(aq)çè2Ag+(aq) +
H2S(aq)
If we start with 2M AgNO3, and .1M H2S, 2M
HNO3 , and 25.g of Ag2S in which direction
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14-3) The reaction H3PO4(aq) +
3OH-(aq) ↔ 3H2O(l) +
PO4(aq)3- is exothermic. What will happen
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a)...

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Calculate the value of Kp for the reaction, 1/2 Cl2(g) + 1/2
I2(g) <=> ICl(g)
5) Calculate Kc for the following reaction,
H2(g) + I2(g) <=> 2 HI(g);
Kp = 97.5 at 25.0 o C

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