consider the following system at equilibrium: SiF4 (g) + 2H2O + heat 《》SiO2 (g) + 4HF...

consider the following system at equilibrium:
SiF4 (g) + 2H2O + heat 《》SiO2 (g) + 4HF (g)

a. Is this reaction endothermic or exothermic?
b Which direction will the equilibrium shift if HF is added?
c. Which direction will the equilibrium shift if H20 is removed?
d. Which direction will the equilibrium shift if the system is heated?

Expert Solution

From Le Chatelier's principle

1.If there are more moles of reactants, an increase in volume will shift the equilibrium to the left in order to favor the reactants. When there is a decrease in volume, the equilibrium will shift towards the side of the reaction with fewer moles.

2. When there is a decrease in pressure, the equilibrium will shift towards the side of the reaction with more moles of gas.When there is an increase in pressure, the equilibrium will shifttowards the side of the reaction with fewer moles of gas.

3. For an exothermic reaction, if you increase the temperature you are increasing the amount of products, and so you shift the balance at equilibrium back toward reactants.

4. If you add reaction products to a chemical system at equilibrium, you can expect that some amount of product will be converted into reactants, while if you add reactants, some amount of reactants will be converted into products so that equilibrium is maintained.

So answer is

queen_honey_blossom answered 1 year ago

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