Question

Review Intelligent Tutoring Problem 6.65 A 1.000 mol sample of propane, a gas used for cooking in many rural areas, was placed in a bomb calorimeter with excess oxygen and ignited. The initial temperature of the calorimeter was 25.000 °C and its total heat capacity was 97.13 kJ °C-1. The reaction raised the temperature of the calorimeter to 27.282 °C. Write the balanced chemical equation for the reaction in the calorimeter. How many joules were liberated in this reaction? What is the heat of reaction of propane with oxygen expressed in kilojoules per mole of C3Hg burned? Part 1 X Incorrect. Do you have the correct product of carbon dioxide and water? Are there equal numbers of atoms on either side of the equation? The first step in solving this problem is to find the balanced equation. Write the balanced equation for this reaction below. Include physical states in your answer C2H2 +502 — 3C02 + 4H20 Edit

Answer 1

n=C₃ Hg = 1.000 mol AT = 27.282°C -25°C 52.282°C c=97.13 kJ / a) Balanced equation .. C3 HQ +502 -> 300, + 4H20 b) Q = ? Q = C.ot - 97-13k, 2.2828 q = 221.650 ki c) DHC -kj - 221.65oks = 221.65 kJ/mol. 1000 mol