The goal of this lesson:
Evaluate experimental results showing equilibria shifts due to temperature change
Using this reversible reaction, answer the questions below:
N2O4 2NO2
(colorless) (reddish-brown)
-As the temperature increased, what happened to the N2O4 concentration?
-Was the formation of reactants or products favored by the addition of heat?
-Which reaction is exothermic? Right to left or left to right?
-If the change of enthalpy of this reaction when proceeding left to right is 14 kcal, which chemical equation is correct?
N2O4 2NO2 + 14 kcal
N2O4 2NO2, HR = +14 kcal
N2O4 + 14 kcal 2NO2
N2O4 2NO2, HR = -14 kcal
Answers: 3
Chemistry, 22.06.2019 00:10
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Answers: 1
Chemistry, 22.06.2019 08:30
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Consider the following reaction at equilibrium. 2co2 (g) 2co (g) + o2 (g) h° = -514 kj le châtelier's principle predicts that the equilibrium partial pressure of co (g) can be maximized by carrying out the reaction a. at high temperature and high pressure b. at high temperature and low pressure c. at low temperature and low pressure d. at low temperature and high pressure e. in the presence of solid carbon
Answers: 2
The goal of this lesson:
Evaluate experimental results showing equilibria shifts due to temperature...
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