Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. M₂O3(s) = 2M(s) + 1º₂(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? AGrxn 10.3 = What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? 0.0156 K = What is the equilibrium pressure of O2 (g) over M(s) at 298 K? 1.0267 Po₂ Incorrect Substance AG (kJ/mol) M2O3(s) -10.30 M(s) 0 02(g) 0 kJ/mol bar

Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. M₂O3(s) = 2M(s) + 1º₂(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? AGrxn 10.3 = What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? 0.0156 K = What is the equilibrium pressure of O2 (g) over M(s) at 298 K? 1.0267 Po₂ Incorrect Substance AG (kJ/mol) M2O3(s) -10.30 M(s) 0 02(g) 0 kJ/mol bar

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the equilibrium constant k for the following reaction at 75 degree C A2 + B2 > 2AB Given Delta H(kJ/mol) DeltaS(J/mol K) A2 0 119 B2 0 125 AB 0 292 Write your answer in exponential form
Calculate AG for H,O(g)+½O¸ (g) =H,O, (g) at 600.0 K, using the following data: H2e) + O28) = Kp = 2.3 x106 at 600.0 K Kp = 1.8 x 1037 at 600.0 K H202(9) 2H2(g) + O28) = 2H20(g)
BaCl, · H,O(s) loses water when it is heated in an oven: BaCl, · H,O(s) = BaCl, (s) + H,O(g) AH° = 63.11 kJ/mol at 25 °C AS +148 J/(K · mol) at 25 °C Write the equilibrium constant for this reaction. Find the vapor pressure of H,O (PH,0) above BaCl, · H,O(s) at 298 K. PH,0 bar = If AH° and AS° are not temperature dependent (a poor assumption), estimate the temperature at which PH,0 above BaCl, · H, O(s) will be 1 bar. T = °C
At 13.7 °C the concentration equilibrium constant K = 2.0 × 10 for a certain reaction. Here are some facts about the reaction: • C The constant pressure molar heat capacity C₁ = 2.49 J-mol K. •If the reaction is run at constant pressure, 147. kJ/mol of heat are released. •If the reaction is run at constant pressure, the volume increases by 13.%. ○ Yes. Using these facts, can you calculate K, at 3.8 °C? x10 No. If you said yes, then enter your answer at right. Round it to 2 significant digits. n If you said no, can you at least decide whether Kat 3.8 °C will be bigger or smaller than K at -13.7 °C? Yes, and K will be bigger. Yes, and K will be smaller. No. x
Gg.124.
The following reaction takes place into a constant-volume flask at 427°C: CCL(g) = C(s) +2 C2(g) AH=132 kJ At 427°C, the equilibrium constant for the reaction given above is K. = 1.3×10-2. A flask is filled with 2.00 atm of CCl4 at 427°C. (a) What is the value of K for this reaction? (R=0.082 L.atm/mol.K) (b) What are the partial pressures of CClL, Ch and the total pressure at equilibrium? (c) How will the equilibrium pressure of CCl(g) change if the temperature is increased? (d) How will the equilibrium system respond if the volume of the flask is reduced?
Kp for the following reaction is 0.16 at 25 0C. 2NOBr(g)=2NO (g)+ Br2 (l) the enthalpy change for the reaction at standard conditions is +16.1 kJ. State which way the equilibrium will shift (left, right or no change) when each of the following changes is made. Breifly explain credit for result. (a) adding more Br2 (l) (b) removing some NOBr (g) (c) Decreasing the temperature (d) increasing the container volume (e) increasing the total pressure by adding an inert gas.
Calculate AG°for each of the following reactions from the equilibrium constant at the temperature given. Reaction Temperature (°C) 2000 N₂ (g) + O₂(g) →→→ 2NO (g) H₂ (g) + 12 (g) → 2HI (g) 400 CO₂ (g) + H₂ (9) → CO (g) + H₂O (g) 980 CaCO3 (s) → CaO (s) + CO2 (g) 900 Ko value 4.1 x 10-4 50.0 1.67 1.04
The equilibrium constant, Kċ, for the following reaction is 1.29×10-² at 600 K. Calculate Kp for this reaction at this temperature. COCI₂(g) ⇒CO(g) + Cl₂(9) Кр || =
What is the increment G degree for the following reaction from the equilibrium constant at the temperature given? CaCO33(s) → CaO(s) + CO2(g)T = 900°C Kp= 1.04
Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g) + O2(g) ⇆ 2NO(g) is 0.010. If 0.40 moles of N2, 0.10 moles of O2, and 0.080 moles of NO are placed in a 1.0-liter container, what will be the concentration of O2 at equilibrium?
The value of the equilibrium constant K, for the reaction below is 0.649 at 900°C. H, (g) + CO,(g) = = H,0(g) +CO(g)