This problem set is due at $10$ am on Nov. $10,2023.$

Please be sure to show all work, including units, for each step of the problem. Pay careful

attention to sig figs.

The specific heat capacity of water is $4\mathrm{.}18\frac{J}{g}C.$ The value is also $4\mathrm{.}18\frac{J}{g}K.$ Explain

why no conversion factor for heat capacity is necessary when changing the temperature unit

system between Celsius degrees and kelvin.

Question $6\mathrm{.}48$ on page $285$ of your text. Hints: $1.$ use the limiting reactant to determine

the moles of reaction present in the experiment. $2.$ In this experiment, the system $($reaction$)$

is placed inside the surroundings $($the aqueous solution$)$ rather than underneath it like in

the combustion reaction from class. To determine $q_{\text{s}\text{u}\text{r}\text{r}},$ use the entire mass of the solution.

You can get the entire mass of the solution from the volumes of the components given at

the beginning of the problem. $3.$ Express your calculated value of $H$ in units of $k\frac{J}{m}ol$

rxn$,$ rather than $k\frac{J}{m}$olAgCl as suggested in the text.

Consider the following thermochemical equation:

$S_8+8H_{2}8H_{2}S,H=-20\mathrm{.}2k\frac{J}{m}$olrxn

a$.$ Determine $q_{sys}$ if $0\mathrm{.}500mol{H}_{2}S$ is produced.

b$.$ Determine $q_{sys}$ when $25\mathrm{.}0g$ of $S_8$ and $25\mathrm{.}0g{H}_2$ are available to react. Hint: determine

the limiting reagent first.

c$.$ Determine the mass of $H_{2}S$ produced if $10\mathrm{.}0kJ$ is released in the reaction.

Use the database of calorimetric measurements below, along with Hess' Law, to calculate

the value of $H($in $k\frac{J}{m}$olrxn

and water vapor:

$2C_2{H}_2+5O_{2}4C{O}_2+2H_{2}O.$

$C_2{H}_{2}2C+H_2$;$H=-226\mathrm{.}88k\frac{J}{m}$olrxn

$C{O}_{2}C+O_2$;$H=+393\mathrm{.}5k\frac{J}{m}$olrxn

$H_{2}O{H}_2+\frac{1}{2}{O}_2$;$H=+241\mathrm{.}82k\frac{J}{m}$olrxn