The following reaction has been allowed to come to equilibrium in a 2.0 L contai

Question

The following reaction has been allowed to come to equilibrium in a 2.0 L container 2 Cl_2 O(g) 2 Cl_2(g) + O_2(g) + energy State the direction in which the equilibrium would be shifted (Right, Left, or unchanged) Upon application of the following " ": Increase the concentration of Cl_3O _____ Increase the concentration of O_1 _____ Decrease the concentration of Cl_2 _____ Increase the pressure by decreasing the volume to 1.0 L _____ Increase the temperature _____ Add s catalyst _____ Add He(g) to the 2.0L container _____ The following system has been allowed to come to equilibrium at 25 degree C. AgC_2H_2 O_2() Ag^+ C_2H_2O_2^- State the direction in which the equilibrium will be shifted if the following are added to 1.0 L of the equilibrium mixture: Solid AgNO_3 _____ Solid NaC_2M_ O_2 _____ 6 M HNO_3 _____ Solid AgC_2H_3O_2 _____ 100 mL of H_2O _____ predict whether the following salts which are insoluble in water would be by addition a strong acid, such as HNO_3. If solution occurs, write the net equation for the reaction. MgCO_3 _____ _____ AgCl _____ _____ Ca_3(PO_4)_2 _____ _____ ZnS _____ _____ BaSO_4 _____ _____

Explanation / Answer

Q1.

2Cl2O = 2Cl2 + O2 + heat

this is exothermic, releases heat

so..

Q1

First, let us state the Le Chatelier principle which deals with changes in an equilibrium:

The statement is as follows:

If any equilibrium is disturbed, that is, change in conditions such as P,T, concentration, partial pressure, etc.., the system will counterbalance such change in order to favour the system's equilbirium.

Now, knowing this:

Q1.

increase of Cl2O will favour more Cl2 and O2 production, it shifts toward RIGHT

Q2.

icnrease in O2, a product, favours more Cl2O production, so shift goes toward LEFT

Q3.

Decrease in product makes the shift go toward even MORE produicts, so it goes to RIGHT

Q4.

Increase in prsesure favours the LEAST mol of gas formation, this is Cl2O, so shift goes toward REACTANTS, LEFT

Q5.

increase in T, will not favour this, since it is exothermic, so this favours Cl2O, the reactants, it goes to LEFT

Q6.

catlayst will only increase rate not equilibrium, NO EFFECT

7

addition of an inert gas increases pressure, similar as to 4, the shift goes toward more reactants

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