Consider the following equilibrium reaction: Cl2(g) + PCl3(g) PCl5(g) Initial concentrations of Cl2 and PCl3 are shown in the following data table and the concentration changes at various time periods after the reaction has started. Reaction Time Cl2 (mol/L) 0s 20 s 40 s 60 s 80 s 100 s 120 s
2.
1.00 0.90 0.80 0.75 0.71 0.71 0.71
PCl3 (mol/L)
PCl5 (mol/L)
1.00 0.90 0.80 0.75 0.71 0.71 0.71
0.00 0.10 0.20 0.25 0.29 0.29 0.29
a)
When was equilibrium attained? ________________
b)
What would the concentration of Cl2 be after 20 hours? ________________
c)
After 40 s which reaction (forward or reverse) is faster? ________________
d)
At 25 s is the forward reaction increasing or decreasing in its rate? ________
e)
At 25 s is the reverse reaction increasing or decreasing in its rate? _________
f)
At 100 s which reaction is faster, forward or reverse? ________________
g)
At 100 s which reaction is increasing in rate, the forward or the reverse? ________________
Give an example of a reaction that "goes to an end" from your experience. ______________________________________________________________________
3.
Can all reactions attain a state of equilibrium? Why or why not? ______________________________________________________________________
1
2 4.
a)
Use the following graph to determine:
i)
the equilibrium concentrations of N2(g) ____________, H2(g) ____________, and NH3(g) ____________.
ii)
the time taken to reach equilibrium: _________________
b)
Which reaction (f) or (r) is faster after 10 minutes?
c)
Which reaction (f) or (r) is increasing in rate after (i) 20 min. _________________ and (ii) after 40 min._____________________
4.
When equilibrium is reached through the decomposition of HBr (aq) at high temperatures, how do the amounts of each product compare? ________________________________ Is this true for the decomposition of NH3? Explain. ______________________________________________________________________
requires a ______ ______ where nothing leaves or enters the system. - No net change in concentration of reactants or products occurs. - Quantities of reactants and products are usually not equal (only the speeds of the. forward and reverse reactions
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When writing equilibrium expressions, reactants or products that are pure solids ... Since Kc represents the system at equilibrium, only these concentrations can.
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