Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 g of sucrose, C12H22O11, was burned in a bomb...

Consider the reaction

C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l)

in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C. Calculate the change in internal energy, ΔE, for this reaction per mole of sucrose.

Express the change in internal energy in kilojoules per mole to three significant figures.

Expert Solution

First of all let me start by telling that the heat produced in a bomb calorimeter when combusting a given amount of known substance is the internal energy of the substance combusted per the number of moles of the substance that was burned.

now, findng the number of moles of sucrose:

Here 10.0 g of sucrose is (10.0 g of sucrose) / (342.3 g/mol) = 0.02921 moles of sucrose

You are given that the heat capacity of the calorimeter is 7.50 kJ/ deg C.

This means that the temperature of calorimeter increases 1 deg C when 7.50 kJ of heat is absorbed by the calorimeter from the combustion process. Since the temperature increase was 22.0 deg C when combusting the 0.02921 moles of sucrose, then the combustion process must have given off (22.0 deg C)(7.50 kJ/deg C) = 165.0 kJ..

Therefore, the change in internal energy per mole of sucrose combusted would be = (165.0 kJ) / (0.02921 moles of sucrose combusted) = 5649 kJ/mol of sucrose combusted

queen_honey_blossom answered 2 hours ago

3.11 g of toluene (C7H8) is burned in a bomb calorimeter. The following reaction occurs. C7H8(l)...

3.11 g of toluene (C7H8) is burned in a bomb calorimeter. The following reaction occurs. C7H8(l) + 9 O2(g) → 7 CO2(g) + 4 H2O(l) The temperature of the calorimeter changes from 24.2°C to 40.1°C. Given that the heat capacity of the calorimeter is 8.32 kJ/°C, find the amount of heat generated per mole of toluene. ___ kJ/mol toluene

If 3.305 g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K,...

If 3.305 g of ethanol C2H5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 97.70 kJ . A) Calculate ΔH∘combustion for ethanol at 298.15 K B) Calculate ΔH∘f of ethanol at 298.15 K.

(c) Hydrolysis of sucrose, S (C12H22O11), to glucose, G (C6H12O6) and fructose, F (C6H12O6), in dilute...

(c) Hydrolysis of sucrose, S (C12H22O11), to glucose, G (C6H12O6) and fructose, F (C6H12O6), in dilute aqueous solution is given by: S + H2O -> G + F (i) If the reaction has one elementary step as outlined above, what would be the order of this reaction? Explain your answer. (ii) Outline the differential and the integrated reaction rate laws. (iii) The concentration of sucrose at time zero was 0.01 mol L -1 and at time 200 s 0.004 mol...

A 17.5 g sample of a candy bar is burned in a bomb calorimeter, which has...

A 17.5 g sample of a candy bar is burned in a bomb calorimeter, which has a heat capacity of 9.25 kJ/°C. The temperature increases from 19.7°C to 57.3°C. What is the fuel value of the candy bar? In kJ/g How many Calories are in a 77.7 g candy bar? 1 Cal = 4.184 kJ. In Cal

Table salt, NaCl(s), and sugar, C12H22O11(s), are accidentally mixed. A 3.50-g sample is burned, and 2.10...

Table salt, NaCl(s), and sugar, C12H22O11(s), are accidentally mixed. A 3.50-g sample is burned, and 2.10 g of CO2(g) is produced. What was the mass percentage of the table salt in the mixture?

Table salt, NaCl(s), and sugar, C12H22O11(s), are accidentally mixed. A 6.00-g sample is burned, and 2.80...

Table salt, NaCl(s), and sugar, C12H22O11(s), are accidentally mixed. A 6.00-g sample is burned, and 2.80 g of CO2(g) is produced. What was the mass percentage of the table salt in the mixture?

a 5.00 g sample of TNT (C7H5N2O6) is burned in a bomb calorimeter with a heat...

a 5.00 g sample of TNT (C7H5N2O6) is burned in a bomb calorimeter with a heat capacity of 420 J/degreeC. The calorimeter contained 610 grams od water (4.18J/gdegreeC) and the temperature of the water was measured to go from 20.0 degree C to 22.5 degree C. What is the heat of combustion of TNT?. I know the answer, but can you give me a step by step explanation of how to get it?

A concentrated solution of sucrose, C12H22O11, contains 233.2 g dissolved in 397.07 g water. The density...

A concentrated solution of sucrose, C12H22O11, contains 233.2 g dissolved in 397.07 g water. The density of the solution is 1.1507 g mL-1 Calculate; weight percent, mol fraction, molality, and molarity of C12H22O11 in the solution

A) A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.423 kg of water....

A) A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.423 kg of water. The final volume of the solution is 355 mL. 1) For this solution, calculate molarity. 2) For this solution, calculate molality. 3) For this solution, calculate percent by mass. 4) For this solution, calculate mole fraction. B) Calculate the vapor pressure at 25 ∘C of a solution containing 55.2 g ethylene glycol (HOCH2CH2OH) and 286.6 g water. The vapor pressure of pure water at...

A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.394 kg of water. The...

A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.394 kg of water. The final volume of the solution is 355 mL. calculate: a- molarity b- molality c- percent by mass d- mole fraction

Question