Equilibrium and LeChatelier\'s Principle Pre-laboratory Questions Using LeChartl
ID: 537726 • Letter: E
Question
Equilibrium and LeChatelier's Principle Pre-laboratory Questions Using LeChartlier's principle, determine whether the reactants or products are favored and the direction of the shift in equilibrium (left or right) in the following examples. 2CO(g) + O_2(g) rightarrow 2CO_2(g) + heat Equilibrium and LeChatelier's Principle Laboratory Questions Common Ion Effect What is the "common ion" that you added to test tubes #2-5? How does the common ion effect the equilibrium reaction as the amount of NaCI solution increases from 1-4 mL? Equilibrium and LeChartlier's Principle Consider the following equilibrium reaction for the production of sulfur trioxide. a. write a balanced equation with the heat value on the proper side of the equation. b. Determine the shift in equilibrium (left or right) and if the concentration of the reactants or products increases in the following examples. Adding more SO_3 Removing heatExplanation / Answer
1. For the given reaction:
2CO (g) +O2 (g) ------ 2CO2 (g) + heat
The forward reaction is exothermic as heat is evolved and its included as a product.
The position of equilibrium will shift to the right. More reactants are converted into products at the lower temperature. Thus the products are favoured.
Next page question is incomplete because we need to know what you taking in the test tubes 2-5.
2. (a) balanced equation with heat value:
2SO2 (g) + O2 (g) ===== 2SO3 (g) + 196.6 kJ
(b) Adding more SO3 indicates the increasing the concentration of product, thus the equilibirium position shifts to left side to reduce the product concentration.
Removing heat equilibrium shifted to the left side because the reaction will endothermic.
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