62 The oxidation of glucose, C,H,,Oc, to carbon dioxideand water is exothermic. The heat liberated is thesame whether glucose is metabolized in the body orburned in air.12C,H12O6 + 602> 6CO2 + 6HO + 670 kcalGlucoseCalculate the heat liberated when 15.0 g of glucose ismetabolized to carbon dioxide and water in the body.

Answered: Image /qna-images/answer/963e317c-ef88-421b-bc3b-6d11dea23ea0.jpg

62 The oxidation of glucose, C,H,0, to carbon dioxide 12 69, and water is exothermic. The heat liberated is the same whether glucose is metabolized in the body or burned in air. C6H12O6 + 602 6CO2 + 6H,O + 670 kcal Glucose Calculate the heat liberated when 15.0 g of glucose is metabolized to carbon dioxide and water in the body.

62 The oxidation of glucose, C,H,0, to carbon dioxide 12 69, and water is exothermic. The heat liberated is the same whether glucose is metabolized in the body or burned in air. C6H12O6 + 602 6CO2 + 6H,O + 670 kcal Glucose Calculate the heat liberated when 15.0 g of glucose is metabolized to carbon dioxide and water in the body.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium chloride(s). HCl(g) + NH3(g) --> NH4Cl(s) ΔH = -176kJ How many grams of HCl(g) would have to react to produce 45.2 kJ of energy? _______ grams
A 138.9 g sample of an unknown metal at a temperature of 99.1 °C is added to 44.72 g of water at a temperature of 19.1 °C. The specific heat of water is 4.184 Jg-1 °C- 1. The final temperature of the system is 52.2°C. Calculate the specific heat of the unknown metal.
How much energy is required to decompose 1970 g of PCl3, according to the reaction below? 4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°RXN = +1207 kJ
100.0 ml of 0.115 m potassium hydroxide solution is mixed with 75.0 ml of 0.245 M nitric acid solution in a coffee cup calorimeter. Before mixing, both solutions are initially at 23.85 C;after mixing, the temperature of the mixture in the coffee cup calorimeter increases to 26.30 C. Determine the enthalpy change(delta h) of reaction in kJ/mol for the reaction as written below. KOH(aq) + HNO3(aq) ⮕ KNO3(aq) + H2O(aq) Assume the resulting solution density is 1.03 g/mL. Specific heat of solution=4.20 J/g C
A chemist carefully measures the amount of heat needed to raise the temperature of a 286.0 g sample of a pure substance from 6.3 °C to 23.4 °C. The experiment shows that 11.9 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits. - ·K
Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.80 x 10² kJ of heat? The balanced chemical equation is as follows: C(s) + O2 (g) → CO2 (g), Express the mass in grams to three significant figures. VE ΑΣΦ m = ? g AHxn=-393.5 kJ
A piece of molybdenum metal whose mass is 6.87 g is heated to 100.0 °C and then dropped into an ice calorimeter. As the molybdenum cools to 0.0°C, 0.513 g of ice melts (it takes 6.01 kJ of heat to melt exactly 1 mol of ice). What is the molar heat capacity (in J/mol·K) of molybdenum? i J/mol*K
We allow 81 g of oxygen to react with 66 g of ethane. The reaction is shown below. Since the heat of combustion of ethane is -1560 kJ/mol, how much heat is exchanged by the system if the reaction is the system? C2H6 (g) + 72 O2 (g) → 2 CO2 (g) + 3 H2O (g)
The heat of reaction for the combustion of benzene (C6H6) is –3909.9 kJ. 2 C6H6 15 O2 → 12 CO2 + 6 H20 What would be the heat change when 161.54 g of benzene is burned in kilojoules?
2. A piece of Cu metal is heated in a test until the temperature reaches 96 °C and dropped into a calorimeter with 50.0 ml of water with a temperature of 27°C. after the addition of the metal, temperature of water in the calorimeter rises to 29 °C What is the mass of Cu added?
At constant volume, the heat of combustion of a particular compound is −3733.0 kJ/mol.−3733.0 kJ/mol. When 1.361 g1.361 g of this compound (molar mass=185.51 g/mol)(molar mass=185.51 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 8.567 ∘C.8.567 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?
Please answer question 18 part A