This problem set is due at $10$ am on Friday, Dec. $1,2023.$

Problem $16\mathrm{.}65$ on page $738$ of your textbook. Also: use the units of the rate constant

to determine the overall order of the reaction $($sum of exponents $m+n).$

Sulfur trioxide decomposes at high temperature in a sealed container:

$2S{O}_3(g)2S{O}_2(g)+O_2(g)$

Initially the container at $1000K$ contains only $S{O}_3,$ at a concentration of $6\mathrm{.}09{10}^{-3}$

$M.$ At equilibrium, the $S{O}_3$ concentration is $2\mathrm{.}44{10}^{-3}M.$ Calculate the value of $K_c$ at

$1000K.$

For the reaction $H_2(g)+I_2(g)2HI(g),K_c=55\mathrm{.}3$ at $700K.$ In a $2\mathrm{.}00-$L flask containing

an equilibrium mixture of the three gases, there are $0\mathrm{.}056g{H}_2$ and $4\mathrm{.}36g{I}_2.$ What is the

mass of $HI$ in the flask?

Problem $17\mathrm{.}55$ on p$.789$ of your text.

When solid $N{H}_{4}HS$ and $0\mathrm{.}400$ mole of gaseous $N{H}_3$ were placed into a $2\mathrm{.}0-$L container

at $24C,$ the equilibrium $N{H}_{4}HS(s)N{H}_3(g)+H_{2}S(g)$ was reached. For this reaction,

$K_c=1\mathrm{.}6{10}^{-4}.$ What are the equilibrium concentrations of $N{H}_3$ and $H_{2}S?$