91影视

Balance each reaction and write its reaction quotient, ${\mathbf{Q}}_{\mathbf{c}}$:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{}\mathbf{NO}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{N}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{}{\mathbf{SF}}_{\mathbf{6}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{SO}}_{\mathbf{2}}{\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{}{\mathbf{SCIF}}_{\mathbf{5}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{S}}_{\mathbf{2}}{\mathbf{F}}_{\mathbf{10}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{HCI}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \end{gathered}$$

Balance each reaction and write its reaction quotient, ${\mathbf{Q}}_{\mathbf{c}}$:

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{}\mathbf{}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{6}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}\mathbf{}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{}{\mathbf{CH}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{F}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{CF}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{4}\mathbf{HF}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{,}\mathbf{} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{SO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{G}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{,}\mathbf{} \end{gathered}$$

Balance each reaction and write its reaction quotient,${\mathbf{Q}}_{\mathbf{C}}$ :

$$\begin{gathered} \mathbf{\left(}\mathbf{a}\mathbf{\right)}\mathbf{}{\mathbf{NO}}_{\mathbf{2}}\mathbf{CI}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}\mathbf{}{\mathbf{NO}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{CI}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathbf{}{\mathbf{POCI}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{PCI}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \\ \mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}\mathbf{}\mathbf{饾啅}\mathbf{}\mathbf{}{\mathbf{N}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{g}\mathbf{\right)} \end{gathered}$$

101 The methane used to obtain ${\text{H}}_2$ for manufacture is impure and usually contains other hydrocarbons, such as propane,${\text{C}}_3{\text{H}}_8$ . Imagine the reaction of propane occurring in two steps:

$\begin{array}{l}{\text{C}}_3{\text{H}}_8\left(g\right)+3{\text{H}}_2\text{O}\left(g\right)鈬�3\text{CO}\left(g\right)+7{\text{H}}_2\left(g\right)\\ K_{\text{p}}=8.175脳{10}^{15}\text{at}1200\text{K}\\ \\ \text{CO}\left(g\right)+{\text{H}}_2\text{O}\left(g\right)鈬�{\text{CO}}_2\left(g\right)+{\text{H}}_2\left(g\right)\\ K_{\text{p}}=0.6944\text{at}1200\text{K}\end{array}$

(a) Write the overall equation for the reaction of propane and steam to produce carbon dioxide and hydrogen.

(b) Calculate$K_{\text{p}}$ for the overall process at 1200K

(c) When$1.00$ volume of ${\text{C}}_3{\text{H}}_8$and $4.00$volumes of${\text{H}}_2\text{O}$ , each at$1200.\text{K}$ and$5.0\text{atm}$ , are mixed in a container, what is the final pressure? Assume the total volume remains constant, that the reaction is essentially complete, and that the gases behave ideally.

(d) What percentage of the${\text{C}}_3{\text{H}}_8$ remains unreacted?

Using ${\text{CH}}_4$and steam as a source of${\text{H}}_2$for${\text{NH}}_3$synthesis requires high temperatures. Rather than burning${\text{CH}}_4$separately to heat the mixture, it is more efficient to inject some${\text{O}}_2$into the reaction mixture. All of the${\text{H}}_2$is thus released for the synthesis, and the heat of reaction for the combustion of${\text{CH}}_4$helps maintain the required temperature. Imagine the reaction occurring in two steps:

$\begin{array}{l}2{\text{CH}}_4\left(g\right)+{\text{O}}_2\left(g\right)鈬�2\text{CO}\left(g\right)+4{\text{H}}_2\left(g\right)\\ K_{\text{p}}=9.34脳{10}^{28}\text{at}1000\text{K}\\ \\ \text{CO}\left(g\right)+{\text{H}}_2\text{O}\left(g\right)鈬�{\text{CO}}_2\left(g\right)+{\text{H}}_2\left(g\right)\\ K_{\text{p}}=1.374\text{at}1000\text{K}\end{array}$

(a) Write the overall equation for the reaction of methane, steam, and oxygen to form carbon dioxide and hydrogen.

(b) What is$K_{\text{p}}$for the overall reaction?

(c) What is$K_{\text{c}}$for the overall reaction?

(d) A mixture of$2.0\text{mol}$of ${\text{CH}}_4,1.0\text{mol}$of,${\text{O}}_2$ and$2.0\text{mol}$of steam with a total pressure of 30atm reacts at 1000K at constant volume. Assuming that the reaction is complete and the ideal gas law is a valid approximation, what is the final pressure?

Mixture of $3.00$volumes of${\text{H}}_2$ and$1.00$ volume of${\text{N}}_2$ reacts atrole="math" localid="1657001296390" ${344}^{掳}\text{C}$ to form ammonia. The equilibrium mixture at 110atm contains $41.49\%{\text{NH}}_3$by volume. Calculate $K_{\text{p}}$for the reaction, assuming that the gases behave ideally.

One mechanism for the synthesis of ammonia proposes that${\text{N}}_2$ and${\text{H}}_2$ molecules catalytically dissociate into atoms:

$\begin{array}{l}{\text{N}}_2\left(g\right)鈬�2\text{N}\left(g\right)log{K}_{\text{p}}=鈭�43.10\\ {\text{H}}_2\left(g\right)鈬�2\text{H}\left(g\right)log{K}_{\text{p}}=鈭�17.30\end{array}$

(a) Find the partial pressure of$\text{N}$ in${\text{N}}_2$ at 1000 and 200atm.

(b) Find the partial pressure of $\text{H}$in${\text{H}}_2$ at 1000 and 600atm.

(c) How many$\text{N}$ atoms and$\text{H}$ atoms are present per litre?

(d) Based on these answers, which of the following is a more reasonable step to continue the mechanism after the catalytic dissociation? Explain.

$\begin{array}{l}\text{N}\left(g\right)+\text{H}\left(g\right)鈫�\text{NH}\left(g\right)\\ {\text{N}}_2\left(g\right)+\text{H}\left(g\right)\text{NH}\left(g\right)+\text{N}\left(g\right)\end{array}$

The molecular scenes below depict the reaction $\mathbf{\text{Y}}\mathbf{鈬�}\mathbf{2}\mathbf{\text{Z}}$ at four different times, out of sequence, as it reaches equilibrium. Each sphere (Y is red and Zis green) represents$\mathbf{0}\mathbf{.}\mathbf{025}\mathbf{}\mathbf{\text{mol}}$ and the volume is$\mathbf{0}\mathbf{.}\mathbf{40}\mathbf{}\mathbf{\text{L}}$ .

(a) Which scene represents equilibrium?

(b) List the scenes in the correct sequence.

(c) Calculate${\mathit{K}}_{\mathbf{\text{c}}}$ .

The oxidation of nitrogen monoxide is favoured at :$\text{457K}$

${\text{2NO(g)+O}}_{\text{2}}\text{(g)}鈬�{\text{2NO}}_{\text{2}}{\text{(g)K}}_{\text{p}}{\text{=1.3脳10}}^{\text{4}}$

(a) Calculate ${\text{K}}_{\text{c}}$at .$\text{457K}$

(b) Find${\text{螖贬}}_{\text{rxn}}^{\text{o}}$ from standard heats of formation.

(c) At what temperature does ${\text{K}}_{\text{c}}{\text{=6.4脳10}}^{\text{9}}$?

The kinetics and equilibrium of the decomposition of hydrogen iodide have been studied extensively:

$\text{2HI(g)}鈬�{\text{H}}_{\text{2}}{\text{(g)+I}}_{\text{2}}\text{(g)}$

(a) At${\text{298K,K}}_{\text{c}}{\text{=1.26脳10}}^{\text{-3}}$for this reaction. Calculate ${\text{K}}_{\text{p}}$.

(b) Calculate${\text{K}}_{\text{c}}$for the formation of $\text{HI}$at $\text{298K}$.

(c)Calculate localid="1657006587824" ${\text{螖贬}}_{\text{rxn}}^{\text{o}}$forlocalid="1657006574683" $\text{HI}$decomposition from ${\text{螖贬}}_{\text{f}}^{\text{o}}$values.

(d) At${\text{729K,K}}_{\text{c}}{\text{=2.0脳10}}^{\text{-2}}$for $\text{HI}$decomposition. Calculate${\text{螖贬}}_{\text{rxn}}$for this reaction from the Vant-Hoff equation.