Consider the following exothermic reaction: SnO_2 + 2CO Sn + 2 CO_2 What directi

Question

Consider the following exothermic reaction: SnO_2 + 2CO Sn + 2 CO_2 What direction will the equilibrium when CO_2 is increased? What direction will the equilibrium shift when CO is decreased? What direction will the equilibrium shift when SnO_2 is increased? What is the equilibrium expression (K) for the above reaction? Draw and label an energy diagram for the above reaction (in question 39). Be sure to label each axis, Delta H, activation energy, products and reactants. Also indicate how the energy diagram would change if you added a catalyst. Draw the Lewis structures for dichloroethane (ClCH_2CH_2Cl) and propane (CH_3CH_2CH_3). Explain why, in details, dichloroethane is a liquid while propane is a gas at room temperature. Discuss specific attractive forces. Write the balanced equation for the electrolysis of water, forming hydrogen and oxygen gas. Draw an energy diagram for this reaction. Which type of reaction was this (combustion, double replacement, acid/base, redox, etc)?

Explanation / Answer

According to le-chatler's principal:

i) when CO2 is increased, the equilibrium will shift towards the left.

ii) When CO is decreased the equilibrium will shift towards the left.

iii) When SnO2 is increased, the equilibrium will shift towards the right.

iv) K={ [SnO2][co]^2}{[sn][CO2]^2}

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