Given these equilibrium reactions: 1. % Sa(s) + 2O2te) <---------- → 2 SO2 Ka = 1.86 x 10105 2. 1/8 Ses) + 3/2 O...
INCLASS EXERCISE ON CHEMICAL EQUILIBRIUM (FINAL) DUE FRIDAY 11/08/2019 NAME Given these equilibrium reactions: 1. X Saw + 2024 <------- 2 SO200) Ka = 1.86 x 10105 2. 1/8 SW + 3/2021) <---.....→ S03e) K = 1.77 x 105 Calculate the equilibrium constant kas for the reaction below, which is important in the formation of acid-rain air pollution. 2 SO260 + 02 -----------------→2 503)
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX: -−297 kJ What is the enthalpy change of the following reaction? 2 SO3 (g) ⟶ 2 SO2 (g) + O2 (g) ΔH3=?
1. Consider the following reaction at equilibrium. 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) a. What will happen if the pressure increased? b. What will happen if the concentration of FeS2(s) is decreased? 2) The following reaction is exothermic: What direction will the equilibrium shift if the following changes are made? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) a) Raising the temperature b) Adding SO3 c) Removing O2 d) Decreasing the volume
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
Given the equilibrium constants for reactions 1 and 2, determine the equilibrium constant for reaction 3. (1) 2H2S (g) + SO2(g) = 3S(s) + 2H2O(g) K=1.00 X 10^5 (2) 3SO2(g) + O2(g) = 2SO3(g) K=11.0 (3) 4H2S(g) + 2SO3(g) = 6S(g) + 4H2O(g) + O2 K=?
(10) 5. Use the given reactions and their enthalpies to determine the AHºrxn for the following reaction: 2 S(x) + 3 O2(g) → 2503(g) Hºrxn - ? Given Reactions and their Standard Enthalpies of Reaction: SO2(g) - S(s) + O2(g) 2 SO2(g) + O2(g) 2 S03(g) AHºrxn = +296.8 kJ Hºrxn = -197.8 kJ (10) 6. Use standard enthalpies of formation (AH°f) to determine AHºrxn for the reaction below. 2 CH3OH(1) + 3 02(g) → 2 CO2(g) + 4H2O(g)
QUESTION 17 1 points [CLO-4] Consider the following equilibrium. 2 SO2(g) + O2 (g) ==== 2 SO3 (8) The equilibrium cannot be established when container [Hint: no need to do any calculations !!! 1.0 mol SO3 (8) is/are placed in a 1.0-L 0.25 mol of SO2 (g) and 0.25 mol of 503 (g) 0.50 mol O2(g) and 0.50 mol SO3 (g) 0.25 mol SO2 (g) and 0.25 mol O2 (g) 0.75 mol SO2 (9)
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given the thermochemical equations below. 2 S(s) + 3 O2(g) =2 SO3(g) AH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) AH° = -197 9 kJ Show all work and calculate to the correct number of sig figs.
balance the reactions
x x He → d. SO2(g) + O2(g) → s0(8) Part 2 (1.3 points) X X Hed. 1,8(8)+ 0,(8) - S0,()+ H20(3) Part 3 (1.3 points) X X. 'Ho - o. H,S(8)+ SO2(g) — Sg(s) + H20(8)