91影视

Explain the difference between a heterogeneous and a homogeneous equilibrium. Give an example of each.

Balance each of the following examples of heterogeneous

equilibria and write its reaction quotient, Qc:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{CO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{I}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{}{\mathbf{NH}}_{\mathbf{4}}\mathbf{CI}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{HCI}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \end{gathered}$$

Balance each of the following examples of heterogeneous()

equilibria and write its reaction quotient, Qc:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{I}\mathbf{\right)}\mathbf{+}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}{\mathbf{H}}_{\mathbf{2}}{\mathbf{SO}}_{\mathbf{4}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{}{\mathbf{KNO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}{\mathbf{KNO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{+}\mathbf{}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{}{\mathbf{S}}_{\mathbf{8}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{}\mathbf{+}\mathbf{}{\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{SF}}_{\mathbf{6}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{} \end{gathered}$$

Question:Balance each of the following examples of heterogeneous

equilibria and write its reaction quotient, Qc:

$$\begin{gathered} \left(a\right)\mathbf{}{\mathbf{NaHCO}}_{\mathbf{3}}\mathbf{}\left(s\right)\mathbf{}\mathbf{}\mathbf{}\mathbf{謴}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}\left(s\right)\mathbf{+}{\mathbf{CO}}_{\mathbf{2}}\left(g\right)\mathbf{}\mathbf{}\mathbf{}\mathbf{+}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(g\right) \\ \left(b\right)\mathbf{}{\mathbf{SNO}}_{\mathbf{2}}\left(s\right)\mathbf{}\mathbf{}\mathbf{}\mathbf{+}\mathbf{}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{}\left(g\right)\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{謴}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{Sn}\left(s\right)\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\left(g\right) \\ \left(c\right)\mathbf{}{\mathbf{H}}_{\mathbf{2}}{\mathbf{SO}}_{\mathbf{4}}\left(I\right)\mathbf{}\mathbf{}\mathbf{}\mathbf{+}\mathbf{}\mathbf{}\mathbf{}{\mathbf{SO}}_{\mathbf{3}}\left(g\right)\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{謴}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}{\mathbf{H}}_{\mathbf{2}}{\mathbf{S}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{7}}\left(I\right) \end{gathered}$$

At ${\mathbf{425}}^{\mathbf{0}}\mathbf{C}\mathbf{,}{\mathbf{K}}_{\mathbf{p}}\mathbf{=}\mathbf{4}\mathbf{.}\mathbf{18}\mathbf{脳}{\mathbf{10}}^{\mathbf{-}\mathbf{9}}$for the reaction

role="math" localid="1655096121156" $\mathbf{2}{\mathbf{HBr}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{鈬�}{\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{Br}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

In one experiment, 0.20 atm of HBr(g), 0.010 atm of${\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$ , and 0.010 atm of${\mathbf{Br}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$ are introduced into a container. Is the reaction at equilibrium? If not, in which direction will it proceed?

The water-gas shift reaction plays a central role in the chemical methods for obtaining cleaner fuels from coal:

${\mathbf{CO}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{鈬�}{\mathbf{CO}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{H}}_{\mathbf{2}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

At a given temperature, Kp = 2.7. If 0.13 mol of CO, 0.56 mol of ${\mathbf{H}}_{\mathbf{2}}\mathbf{O}$, 0.62 mol of ${\mathbf{CO}}_{\mathbf{2}}$, and 0.43 mol of ${\mathbf{H}}_{\mathbf{2}}$ are put in a 2.0-L flask, in which direction, does the reaction proceed?

For a problem involving the catalysed reaction of methane and steam, the following reaction table was prepared:

Explain the entries in the 鈥淐hange鈥� and 鈥淓quilibrium鈥� rows.

(a) What is the basis of the approximation that avoids using the quadratic formula to find an equilibrium concentration?

(b) When should this approximation not be made?

Gaseous ammonia was introduced into a sealed container and heated to a certain temperature:

$\mathbf{2}{\mathbf{NH}}_{\mathbf{3}\left(g\right)}\mathbf{}\mathbf{謴}\mathbf{}\mathbf{}\mathbf{}{\mathbf{N}}_{\mathbf{2}\left(g\right)}\mathbf{}\mathbf{}\mathbf{+}\mathbf{3}{\mathbf{H}}_{\mathbf{2}\left(g\right)}$

At equilibrium, $\left[{\mathrm{NH}}_3\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{0225}\mathbf{}\mathbf{M}\mathbf{}\mathbf{,}\mathbf{}\mathbf{}\left[N_2\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{114}\mathbf{}\mathbf{M}\mathbf{,}\mathbf{}\mathbf{}\mathbf{and}\mathbf{}\left[H_2\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{342}\mathbf{}\mathbf{M}$. Calculate Kc for the reaction at this temperature.

Is K very large or very small for a reaction that goes essentially to completion? Explain.