This question is about carbon dioxide

The food and drink industries use a lot of

carbon dioxide. During summer $2018,$ a

global shortage led to supermarkets

limiting frozen food deliveries and

rationing beer. This is ironic considering

the documented rise of atmospheric $C{O}_2$

levels.

$($a$)($i$)$ Draw dot and cross diagrams for carbon dioxide and carbon monoxide.

$($ii$)$ Calculate the difference in the oxidation state between the carbons in carbon

dioxide and in carbon monoxide.

The English chemist William Henry studied the equilibria when a gas dissolves in a liquid. He

proposed that the concentration of a gas dissolved in a liquid is proportional to the gas' partial

pressure when in the gas phase. The proportionality factor is called the Henry's law constant.

The Henry's law constant for $C{O}_2$ is $3\mathrm{.}3{10}^{-2}mold{m}^{-3}at{m}^{-1}.$

Sealed containers of fizzy drinks contain dissolved $C{O}_2.$ This dissolved $C{O}_2$ is in equilibrium

with a small quantity of gaseous $C{O}_2$ at the top of the container.

$($b$)($i$)$ The partial pressure of $C{O}_2$ gas in a $250c{m}^3$ can of fizzy drink is $3\mathrm{.}0$atm at

$25C.$ What is the concentration of $C{O}_2$ in the fizzy drink?

$($ii$)$ What mass of $C{O}_2$ is dissolved in a $250c{m}^3$ can of fizzy drink?

$($iii$)$ If the can contained only the mass of $C{O}_2$ calculated in part $($ii$)$ as a gas, calculate

the pressure in the can when it is stored at $25C.$

$($iv$)$ Under what conditions would $C{O}_2$ gas be most soluble in water?

Tick the correct option in the answer booklet:

high pressure and low temperature

high pressure and high temperature

low pressure and low temperature

low pressure and high temperature

$($c$)$ The maximum pressure that a can of fizzy drink can withstand is $7$atm. Using the graph

below, determine the maximum temperature at which a can can be stored safely.

One method of industrially manufacturing $C{O}_2$ involves the Haber$-$Bosch process.

$C{H}_4+H_{2}OCO+3H_2$ Step $1$

$N_2+3H_{2}2N{H}_3$ Step $2$

$CO+H_{2}OC{O}_2+H_2$ Step $3$

Ammonia $($the product of Step $2)$ is widely used to produce fertiliser. Fertiliser production is

often stopped over the summer. Combined with the increase in demand for soft$-$drinks during

the hot summer last year, the halt in fertiliser production contributed to the $C{O}_2$ shortage.

In Step $3$ an initial mixture of $40$mol of $CO,20$mol of $H_2,$ and $20$mol of $C{O}_2$ in contact with

$40$mol of steam was allowed to come to equilibrium in a reactor at $1100K.$ At $1100K$ this

reaction has a $K_p$ of $0\mathrm{.}64.$

$($d$)$ Calculate the number of moles of each gas leaving the reactor after equilibration.

The standard enthalpies of formation of $C{O}_{(g)},C{O}_{2(g)}$ and $H_2{O}_{(g)}$ are $-110\mathrm{.}5,-393\mathrm{.}5$ and

$-241\mathrm{.}1kJmo{l}^{-1}$ respectively.

$($e$)$ Calculate the enthalpy of reaction for the reaction between $CO$ and steam to form $C{O}_2$

and $H_2.$