7)
Decreasing volume will increase the pressure which in turn shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle
Here reaction shift to the right.
So, product should have lesser number of gases as compared to reactant.
This is true for option A
Answer: A
8)
Kw is thermodynamics constant.
It can’t predict the rate of ionisation.
Kw value is small and it means that the extent of auto ionisation of water is small.
Answer: D
EY The reaction is at yumunu 7) - 7) of the following equilibria, only will shift...
1) Which reaction will shift to the left in response to a decrease in volume? A) 2 SO3 (8) 2 SO2(g) + O2(8) B) N2(g) + 3H2(g) + 2NH3(g) C) 2H1 (8) H2(g) + 12 (8) D) 4 Fe (8) +32(g) 2 Fe2O3 (s) E) H2 (8) + Cl2(g) 2 HCl (g) Explain 2) Based on Le Châtelier's principle, increasing pressure at constant temperature in the following reaction will not change the concentrations of reactants and products. A) N2 (8)...
muruple choice must be on scantron MOLTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which reaction will shift to the left in response to a decrease in volume? A) 2 SO3 (8) 2 SO2 (8) + O2 (8) B) N2 (8) + 3H2 (8) 2 NH3 (8) C) 2HI (8) H2(g) + 12 (g) D) 4 Fe (s) + 3 O2 (g) 2 Fe203 (s) E) H2 (8) + Cl2 (8) 2...
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
Arrange the following gases in order of decreasing standard molar entropy: N204(9), NO(g), NO2(g). Select one: O a. N204> NO > NOZ O b. N204 > NO2 > NO O C. NO2 > NO > N20. O d. NO > NO2 > N204 e. NO > N204 > NO2 Which of the following reactions will shift to the left if the volume is decreased? Select one: H2 (8) + Cl2 (8) DIL 2 HCI (8) OD b. 2 SO3 (8)...
14. The following reaction mechanisms are used for the final reaction shown: 203 → 302 Step 1: CI+O3 → 02 + Clo Step 2: 03 → 02 +0 Step 3: ClO +002+CI a. What is the catalyst in the reaction? b. What is/are the intermediate product(s) for the reaction? 15. At a particular moment during the reaction, Hl disappears at a rate of 6.50 X 102 M/s. What is the rate of appearance of H2 and the rate of appearance...
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2(g) 02(8)2 S03(g) O A) Adding SO3 O B) Increase volume O c) Increase the temperature OD) Adding catalyst 0 E) Increase pressure
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...
52) Use the standard reaction enthalpies given below to determine AHryn for the tonowe reaction P4() + 10 C12(e) → 4PC15(s) Hºrxn = ? Given: PC15(s) → PC13(g) + Cl2(e) AHørxn = +157 kJ P4(B) + 6 Cl2(e) → 4 PC13(g) AH*rxn=-1207 kJ A) -1835 kJ B) -1364 kJ C) -1050. kJ D) -1786 kJ E) -2100. kJ 53) Use the standard reaction enthalpies given below to determine AHørxn for the following reaction 4 SO3(e) — 4 S(s) + 6...
(1) Find the H for the reaction below, given the following reactions and subsequent H values: 2CO2(g) + H2O(g) → C2H2(g) + 5/202(g) CH2(g) + 2H2(g) → CHg) H2O(g) - H2(g) + 1/20, (g) C2H6(g) + 7/202(g) → 2CO2(g) + 3H2O(g) answer - 235 kJ H =-94.5 kJ H =71.2 kJ H --283 kJ (2) Find the H for the reaction below, given the following reactions and subsequent H values: N2H4(I) + H2(g) + 2NH3(g) N2H4(1) + CH4O(1) - CH2O(g)...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2, each at an intitial partial pressure of 1.70 atm, are introduced into an evacuated vessel at 600 K. PCO = atm PCl2 = atm PCOCl2 = atm B. The equilibrium constant, Kc, for the following reaction is 2.90×10-2 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) Calculate Kc at this temperature for...