le chatelier\'s principle. Determine in which direction the reaction will shift
ID: 894363 • Letter: L
Question
le chatelier's principle. Determine in which direction the reaction will shift in each case. Asumme the system initially is at equilibirum.
a) A (g)+B2 (g)=3C (g)+D (g) pressure is increased
b) A (g) +B (g) = 3C (l) +D (g) volume of vessel is doubled
c) A (g) +B2 (g) = 3C (s) +D (g) exothemic reaction, temperature is increased.
d) A (g) + B (g)= 3C (l) +D (g) endothemic reaction, catalyst is added.
e) A (g) + B2 (g)= 3C (s) +D (g) concentration of D(g) is tripled
f) A (g)+ B2 (g) = 3 C (s) +D (g) Amount is doubled.
g) A (g) +B2 (g) = 3C (g) +D(g) the endothermic gas reaction in a chamber is cooled.
Explanation / Answer
a) IF you increase P, then expect less volume, concnetrations will increase... expect the least number of moles formation. In this case, the shift goes to let (3 moles vs. 4 moles)
b) If you increae volume, the reaction shift to "greater number of moles in gas". In this case, 2 mols of gas go to 1 mol of gas (D). Shift goes to reactants
c) If reaction is exothermic, and you are even more temperature, expect the reaction to shift to the left (reactants) to avoid the reaction from heating too much
d) catalyst has no effct in equilibrium conditions
e) If you increase concentration of a product, expect reactant concentration to increase
f) If you increase both amounts, expect shift to the right (4 moles vs. 2 moles)
g) will tend to form more reactants, the shift will go to reactants (if you cool down, temperature drops)
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