Question

1. given that when, in the reaction above, 1.000 g of c2h4(g) is used in a calorimeter with heat capacity of 1741 j/°c. the temperature rises from 23.63 to 25.38 °c. (calorimetry)

Explanation:

Step1: Calculate the heat absorbed by the calorimeter

The heat absorbed by the calorimeter ($q_{cal}$) is given by the formula $q_{cal}=C_{cal}\Delta T$, where $C_{cal}$ is the heat - capacity of the calorimeter and $\Delta T$ is the change in temperature.
$\Delta T=T_{final}-T_{initial}=25.38^{\circ}C - 23.63^{\circ}C=1.75^{\circ}C$ and $C_{cal}=1741\ J/^{\circ}C$.
$q_{cal}=1741\ J/^{\circ}C\times1.75^{\circ}C = 3046.75\ J$

Step2: Calculate the heat of reaction per gram

The heat of reaction per gram ($\Delta H$) of $C_2H_4$ is the heat absorbed by the calorimeter divided by the mass of $C_2H_4$.
The mass of $C_2H_4$ is $m = 1.000\ g$.
$\Delta H=\frac{q_{cal}}{m}=\frac{3046.75\ J}{1.000\ g}=3046.75\ J/g$

Answer:

$3046.75\ J/g$