Question

In: Chemistry

For the equilibrium 2NO2(g) ⇌ 2NO(g) + O2(g), Kp = 2.0 × 10-2 at 365oC. Suppose...

For the equilibrium 2NO2(g) ⇌ 2NO(g) + O2(g), Kp = 2.0 × 10-2 at 365oC. Suppose 0.0600 mol NO(g), 0.0150 mol O2(g), and 1.60 mol NO2(g) are added to a rigid 2.00-L flask. What is ΔG?

Solutions

Expert Solution

molarity of NO = 0.06 / 2 = 0.03 M

molarity 0f O2 = 0.015 / 2 = 0.0075 M

molarity of NO2 = 1.60 / 2 = 0.8 M

Kp = Kc (RT)^Dn

2 x 10^-2 = Kc x (0.0821 x 638)^1

Kc = 3.82 x 10^-4

ΔGo = - RT ln Kc

         = - 8.314 x 10^-3 x 638 x ln (3.82 x 10^-4)

         = 41.75 kJ/mol

2NO2(g)    <-----------------> 2NO(g) + O2(g)

0.8                                       0.03      0.0075

Qp = [NO]^2[O2] / [NO2]^2

      = 0.03^2 x 0.0075 / 0.8^2

       = 1.05 x 10^-5

ΔG = ΔGo + RT ln Qp

      = 41.75 + 8.314 x 10^-3 x 638 x ln (1.05 x 10^-5)

      = -19 kJ/mol

ΔG = -19 kJ/mol

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

The reaction 2NO(g) + O2(g) ? 2NO2(g) has Kp = 1.65 ×10^11 at 25°C. To a...
The reaction 2NO(g) + O2(g) ? 2NO2(g) has Kp = 1.65 ×10^11 at 25°C. To a 1.00 L flask, 1.03 g of NO and 532 mL of O2 measured at 29°C and 772 torr are mixed. When the mixture comes to equilibrium at 25°C, what is the concentration of NO(g)? If needed, use “E” for scientific notation. Do not enter units as part of your answer. Report your answer to the correct number of significant figures.
The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To...
The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To a 1.00 L flask, 1.03 g of NO and 532 mL of O2 measured at 29°C and 772 torr are mixed. When the mixture comes to equilibrium at 25°C, what is the concentration of NO(g)? If needed, use “E” for scientific notation. Do not enter units as part of your answer. Report your answer to the correct number of significant figures.
The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To...
The reaction 2NO(g) + O2(g) ⇌ 2NO2(g) has Kp = 1.65 × 1011 at 25°C. To a 1.00 L flask, 1.03 g of NO and 532 mL of O2 measured at 29°C and 772 torr are mixed. When the mixture comes to equilibrium at 25°C, what is the concentration of NO(g)? If needed, use “E” for scientific notation. Do not enter units as part of your answer. Report your answer to the correct number of significant figures.
chem:1220 ΔS is positive for the reaction ________. A) 2NO (g) + O2 (g) → 2NO2...
chem:1220 ΔS is positive for the reaction ________. A) 2NO (g) + O2 (g) → 2NO2 (g) B) 2N2 (g) + 3H2 (g) → 2NH3 (g) C) C3H8 (g) + 5 O2 (g) → 3CO2 (g) + 4 H2O (g) D) Mg (s) + Cl2 (g) → MgCl2 (s) E) C2H4 (g) + H2 (g) → C2H6 (g)
Consider the reaction for the production of NO2 from NO: 2NO(g)+O2(g)→2NO2(g) -If 85.5 L of O2(g),...
Consider the reaction for the production of NO2 from NO: 2NO(g)+O2(g)→2NO2(g) -If 85.5 L of O2(g), measured at 34.0 ∘C and 633 mmHg , is allowed to react with 143 g of NO, find the limiting reagent. -If 98.2 L of NO2 forms, measured at 34.0 ∘C and 633 mmHg , what is the percent yield?
For the equilibrium: O2(g) + 2 F2(g) 2 OF2(g) ; Kp = 2.3 x 10–15 Which...
For the equilibrium: O2(g) + 2 F2(g) 2 OF2(g) ; Kp = 2.3 x 10–15 Which ONE of the following statements is true? A) If the reaction mixture initially contains only OF2(g), then at equilibrium, the reaction mixture will consist of essentially only O2(g) and F2(g). B) For this equilibrium, Kc = Kp. C) If the reaction mixture initially contains only OF2(g), then the total pressure at equilibrium will be less than the total initial pressure. D) If the reaction...
The rate of the following reaction was studied: 2NO(g) + O2(g) ⟶ 2NO2(g) The initial concentration...
The rate of the following reaction was studied: 2NO(g) + O2(g) ⟶ 2NO2(g) The initial concentration of NO was 0.500 M. After 3.76 s, the concentration was 0.209 M. What is the average rate of the overall reaction? (Hint: you need to consider the coefficient in front of NO).
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) → 2NO2(g) Initially NO...
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) → 2NO2(g) Initially NO and O2 are separated in two different chambers connected by a valve. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end and calculate their partial pressures. Assume that the temperature remains constant at 25°C. Initial conditions are as follows: NO: 3.99 L, 0.500 atm O2: 1.97 L, 1.00 atm PNO = ???atm PO2 = ???atm...
At a particular temperature Kp = 0.041 for the reaction N2(g) + O2(g) ⇄ 2NO(g) What...
At a particular temperature Kp = 0.041 for the reaction N2(g) + O2(g) ⇄ 2NO(g) What is the equilibrium partial pressure of NO if a flask initially contains 0.12 atm of all three gases? Report the pressure of NO in atm rounded to the nearest hundredth of an atm.
Part A. Calculate the enthalpy of the reaction 2NO(g)+O2(g)?2NO2(g) given the following reactions and enthalpies of...
Part A. Calculate the enthalpy of the reaction 2NO(g)+O2(g)?2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)?NO2(g),   ?H?A=33.2 kJ 12N2(g)+12O2(g)?NO(g),  ?H?B=90.2 kJ Part B. Calculate the enthalpy of the reaction 4B(s)+3O2(g)?2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)?3O2(g)+B2H6(g),    ?H?A=+2035 kJ 2B(s)+3H2(g)?B2H6(g),                            ?H?B=+36 kJ H2(g)+12O2(g)?H2O(l),                ?H?C=?285 kJ H2O(l)?H2O(g),                                          ?H?D=+44 kJ
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT