Question

In: Chemistry

Consider the following equilibrium: N2O4(g)?2NO2(g) Thermodynamic data on these gases are given in Appendix C in...

Consider the following equilibrium:
N2O4(g)?2NO2(g)
Thermodynamic data on these gases are given in Appendix C in the textbook. You may assume that ?H? and ?S? do not vary with temperature.

Part A At what temperature will an equilibrium mixture contain equal amounts of the two gases? Express your answer using four significant figures

Part B

At what temperature will an equilibrium mixture of 1 atm total pressure contain twice as much NO2 as N2O4?

Express your answer using four significant figures.

Part C

At what temperature will an equilibrium mixture of 9 atm total pressure contain twice as much NO2 as N2O4?

Express your answer using four significant figures.

Part D

Rationalize the results from parts B and C by using Le Chatelier's principle (Section 15.7 in the textbook).

Solutions

Expert Solution

queen_honey_blossom answered 3 years ago
Next > < Previous

Related Solutions

Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a...
Consider the following reaction. 2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.722 atm, and N2O4 at a pressure of 0.0521 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO2= ?? atm PN2O4= ?? atm
The equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g)...
The equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? equilibrium, left, right? PNO2 = 0.154 atm, PN2O4 = 0.148 atm...
N2O4 (g) ⇌ 2NO2(g). KP = 0.10 at some Temperature. If 0.40 atm of N2O4 is...
N2O4 (g) ⇌ 2NO2(g). KP = 0.10 at some Temperature. If 0.40 atm of N2O4 is placed in an evacuated flask, what are the pressures at equilibrium?
The half-life for the first-order decomposition of N2O4 is 1.3×10?5s. N2O4(g)?2NO2(g) Part A If N2O4 is...
The half-life for the first-order decomposition of N2O4 is 1.3×10?5s. N2O4(g)?2NO2(g) Part A If N2O4 is introduced into an evacuated flask at a pressure of 19.0 mmHg, how many seconds are required for the pressure of NO2 to reach 1.4 mmHg?
The degree of dissociation, α, for the following reaction: N2O4(g) <--> 2NO2(g) is 0.655 at 298...
The degree of dissociation, α, for the following reaction: N2O4(g) <--> 2NO2(g) is 0.655 at 298 K and 1.00 bar total pressure. Find K.
At 100∘C, Kc = 4.72 for the reaction 2NO2(g)⇌N2O4(g). An empty 10.0 L flask is filled...
At 100∘C, Kc = 4.72 for the reaction 2NO2(g)⇌N2O4(g). An empty 10.0 L flask is filled with 2.30 g of NO2at 100∘C. 1) What is the total pressure in the flask at equilibrium?
The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If...
The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If a reaction vessel at that temperature initially contains 0.030M NO2 and 0.030M N2O4, what are the concentrations of the two gases at equilibrium? First, the reaction quotient (Q) [page 645 of textbook] must be calculated, and then use the I.C.E table [page 648-650 of the textbook] to determine the equilibrium concentrations.
For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) If a reaction vessel initially...
For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K? [N2O4], [NO2] = ____ M
At –80°C, K for the reaction N2O4(g) 2NO2(g) is 4.66 × 10–8. We introduce 0.049 mole...
At –80°C, K for the reaction N2O4(g) 2NO2(g) is 4.66 × 10–8. We introduce 0.049 mole of N2O4 into a 1.0-L vessel at –80°C and let equilibrium be established. The total pressure in the system at equilibrium will be: (0.78 atm)
For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a...
For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K? [N2O4], [NO2] =
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT