Author Question: A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ ... (Read 509 times)

yoroshambo · **on:** Nov 18, 2019

Question 1

The temperature rises from 25.00 °C to 29.00 °C when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate Δ_rU for the combustion of sucrose in kJ mol^-1 sucrose. The heat capacity of the calorimeter is 4.90 kJ °C^-1. The molar mass of sugar is 342.3 g mol^-1.
◦ 1.92 × 103 kJ mol-1
◦ -1.23 × 103 kJ mol-1
◦ -1.92 × 103 kJ mol-1
◦ 2.35 × 104 kJ mol-1

Question 2

A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ °C^-1. Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C. The molar mass of ethanol is 46.07 g mol^-1.

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g)

D_rU = -1235 kJ mol^-1

◦ 74.2 °C
◦ 53.4 °C
◦ 28.1 °C
◦ 111 °C
◦ 85.7 °C

Loise Hard · **Reply #1 on:** Nov 18, 2019

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