# 1.00mol of propene sample is placed in an oxygen filled calorimeter and burned. The starting temperature of the calorimeter is 25.00°C and its total heat capacity is 97.1kJ/°C. The temperature of the calorimeter increased to 27.282°C. Find a), b) and c)?

## a) Chemical equation that balances the reaction in the calorimeter. b) How many J of energy were emitted in this reaction? c) What is the heat released from the reaction of oxygen and propene when burning 1 mol of ${C}_{3} {H}_{8}$

Jun 14, 2018

Here's what I get.

#### Explanation:

(a) The chemical equation

The formula for propene is ${\text{C"_3"H}}_{6}$.

The chemical equation for its reaction with oxygen is

$\text{2C"_3"H"_6 + "9O"_2 → "6CO"_2 + "6H"_2"O}$

(b) Energy released by the reaction

There are two heat transfers to consider:

$\text{heat released by reaction + heat absorbed by calorimeter = 0}$
$\textcolor{w h i t e}{m m m m m m} {q}_{1} \textcolor{w h i t e}{m m m m m l} + \textcolor{w h i t e}{m m m m m m m} {q}_{2} \textcolor{w h i t e}{m m m m m l l} = 0$
color(white)(mmmmmm)q_1color(white)(mmmmml)+ color(white)(mmmmmm)CΔT color(white)(mmmmm)= 0

ΔT = "(27.282 - 25.00) °C = 2.28 °C"

${q}_{1} = \text{-"CΔT = "-97.1 kJ"·color(red)(cancel(color(black)("°C"^"-1"))) × 2.28 color(red)(cancel(color(black)("°C"))) = "-222 kJ}$

(c) Heat released by burning 1 mol of propene

Burning 1 mol of propene releases 222 kJ.