Chapter 13: Q33 E (page 752)
What property of a reaction can we use to predict the effect of a change in temperature on the value of an equilibrium constant?
Changes in enthalpy may be used.
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Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.
Round the following to the indicated number of significant figures:
(a) 0.424 (to two significant figures)
(b) 0.0038661 (to three significant figures)
(c) 421.25 (to four significant figures)
(d) 28,683.5 (to five significant figures)
Question: A 1.00-L vessel at 400 °C contains the following equilibrium concentrations: N2, 1.00M; H2, 0.50M; and NH3, 0.25M. How many moles of hydrogen must be removed from the vessel to increase the concentration of nitrogen to 1.1M?
Calculate the number of moles of \(HI\) that are at equilibrium with \(1.25mol\)of \({H_2}\)and \(1.25\,mol\)of \({I_2}\) in a \(5.00\,L\)flask at \(44{8^0}C\).\({H_2} + {I_2} \rightleftharpoons 2HI\)
\({K_c} = 50.2\,at\,44{8^o}C\)
Cobalt metal can be prepared by reducing cobalt (II) oxide with carbon monoxide.
\(CoO(s) + CO(g) \rightleftharpoons Co(s) + C{O_2}(g)\)
\({K_c} = 4.90 \times 1{0^2}at55{0^o}C\)
What concentration of \(CO\) remains in an equilibrium mixture with \(\left[ {C{O_2}} \right] = 0.100M\)
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