Assume we have an exothermic reaction of a compound $G$ with a base $R,$ both as

aqueous $($in water$)$ solutions. We have $2\mathrm{.}50mL$ of compound $G$ reacting completely

with $7\mathrm{.}50mL$ base R$,$ as per the Method of Variation Set$-$Up Infographic and

Stoichiometry by the Method of Variation Infographic. The initial temperature is at

$30\mathrm{.}9C$ and the final temperature is at $37\mathrm{.}2C.$ Giving a previously determined

calorimeter calibration constant of $a_{\text{c}\text{a}\text{l}}=3\mathrm{.}1$ and assuming $d_{soln}$ and $s_{soln}$ of the

compound $G$ and base $R$ solutions to be the same as those of water

and $s=4\mathrm{.}18\frac{J}{gC},$ calculate $q_{rxn}$ of this chemical reaction between compound G

and base R$.$ Please refer to the Constant$-$Pressure Calorimetry Infographic for all

mathematic equations. Your answer must be have correct significant figures and

correct units to receive credit.

$612J$

$-4820J$

$-816J$

$4820J$

$8\mathrm{.}2{10}^{2}J$

$-8\mathrm{.}2{10}^{2}J$

$4004J$

$204J$

$263J$

$4004J$

$816J$