Question 11Consider the following reaction:Ce2(g) + 2NO(g) = 2NOC{(g)1.1 Determine the estimated value of the equilibrium constant for this reaction at 158 °C by making useof the following data:kjat 25°Cmol)SubstanceS°\mol. Kat 25 °CC{2(g)221.3NO(g)210.890.29NOCE (g)261.751.711.2 Based on your final answer in question 1.1, is the reaction reactant- or product favoured atthis temperature? Use a short sentence to explain your answer.1.3Calculate the value of A,G for this reaction at this temperature, if Cł2 , NO and NOC? arepresent at 0.600 atm, 0.700 atm and 0.500 atm, respectively.

Recall the given equation Cl2g + 2NOg ⇔ 2NOClg Recall the following relations…

Answered: Question 1 1 Consider the following…

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 20QAP

See similar textbooks

Similar questions

Hydrogen iodide gas is formed from its elements with a value for Kp = 25.5 at a certain temperature: H2 (g) + I2 (g) <---> 2 HI (g) What will the equilibrium pressure (in atm) of hydrogen iodide gas be if the initial partial pressure of both reactant gases is 0.150 atm? (answer in 3 significant figures)
Consider the hypothetical reaction, which has an equilibrium constant (Kp) of 16.1 when the reaction occurs at 167°C. 2 W (g) + X (g) <---> 3 Y (g) If the equilibrium partial pressure of W is 0.787 atm and that of Y is 1.65 atm, what will the equilibrium partial pressure (in atm) of X be? (answer in 3 significant figures)
Sulfuryl chloride, SO2Cl2, is a highly reactive gaseous compound. When heated, it decomposes into sulfur dioxide and chlorine. A sample of 3.509 grams of SO2Cl2 is placed in an evacuated 1.00 L bulb and the temperature is raised to 102.0 °C. When the system has come to equilibrium at 102.0 °C, the total pressure in the bulb is found to be 1.43 atm. What is the Kp? (Use ICE table)
Given the equation CH4 (g) + H2O (g) --> CO (g) + 3H2 (g). At 298K, take equilibrium constant K = 1.19x10^-25. At T=1004K, the equilibrium constant is 3.0. At 1004K, the initial partial pressure PCH4 = 30 atm, PH2O = 50 atm and equilibrium is reached at this temperature. After equilibrium is reached, what is the partial pressure and mole fraction of all components?
For a reaction Keq = 17.4 × 10-5 at T = 325 K. What is ΔG° for the reaction?
Calculate K at 298 K for the following reaction: NO(g) + 1/2 O2 (g) <-> NO2 (g) Delta G (kJ/mol) for the following: NO(g) 86.60, NO2(g) 51, O2(g) 0 (answer in scientific notation)
For the following reactionC(??) + 2H2(??) ⇌ CH4(??)K =0.26 at 1000 °C (3 significant figures). What is the equilibrium constant at 750 °C (3significant figures)?
Consider the following equilibrium: N2O4(g) ⇄2NO2(g). If Kp = 0.144 at 950.0 K, calculate Kc. (no scientific notation)
1.1 Determine the value of Kc at 700 degrees Celsius if the gas constant if 8.315Pa m^3 K^-1 mol^-1 1.2 Calculate the value of Kp at 1000 degrees Celsius if the equilibrium concerntration of O2 at 1000 degrees Celsius is 4.6Pa 1.3 is the forward reaction exothermic or endothermic?
For the equilibrium A + B ⇌ C + D K was measured to be 1.51 × 10⁻² at 25°C and 15.0 at 600°C. What is ∆S° for the reaction? Assume ∆H° and ∆S° are temperature independent. Answer in J/mol x K
The following system was set up and allowed to come to equilibrium: 2 NO2(g) ⇌ N2O4 At equilibrium, the concentration of nitrogen dioxide was 2.45 mol/L, and the value of the equilibrium constant for the reaction at that temperature is 0.835. What was the concentration of the dinitrogen tetraoxide? Answer in mol/L to 3 decimal places.
In the reaction 450.0⁰c: caco3(s) ⇌ cao(s) + co2(g), at equilibrium, if pco2 = 0.0160 atm , what is the value of Kc

SEE MORE QUESTIONS

Recommended textbooks for you

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781285199030

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781285199030

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS