The metabolism of glucose (molar mass 180.2 g/mol) with oxygen forms CO, and H,0 and releases 678 kcal/mol of energy. 6 CO2(g) + 6 H,0(1) CGH1206(aq) + 6 O2(g) glucose a. Are the bonds formed in the products stronger or weaker than the bonds broken in the reactants? b. How much energy is released when 4.00 mol of glucose is metabolized? c. How much energy is released when 3.00 mol of O, reacts? d. How much energy is released when 10.0 g of glucose reacts?

The metabolism of glucose (molar mass 180.2 g/mol) with oxygen forms CO, and H,0 and releases 678 kcal/mol of energy. 6 CO2(g) + 6 H,0(1) CGH1206(aq) + 6 O2(g) glucose a. Are the bonds formed in the products stronger or weaker than the bonds broken in the reactants? b. How much energy is released when 4.00 mol of glucose is metabolized? c. How much energy is released when 3.00 mol of O, reacts? d. How much energy is released when 10.0 g of glucose reacts?

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

Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ Reaction 2: 2OF2(g)⟶O2(g)+2 F2(g)ΔH=−49.4 kJ Reaction 3: N2(g)+2O2(g)⟶2NO2(g)ΔH=+66.4 kJ Use Reaction 2. How much energy (in kJ) is released when 79.0 g of oxygen difluoride decomposes?
Nitesh
Calculate the energy change (in kJ) for the combustion of 62.0 grams of propane?
of ld 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) - ►H,O(1) endothermic or exothermic? b) In which direction does heat flow? 175
#24
59.) Gasohol is gasoline mixed with ethanol (C2H5OH). If 0.230 g of ethanol produces 7.24 kJ of energy when burned, what would be the AH for the combustion of one mole of ethanol?
(Q77) The standard Gibbs free energy (AG°rxn) for the formation of sulfur trioxide from sulfur dioxide and oxygen gas is -72.3 kJ/mol. The balanced chemical equation is SO2 (g) + ½ O2 (g) - - SO3 (g). What will be the Gibbs Free energy of the reaction (in kJ/mol) if it takes place at a low temperature of -25.3 °C and the concentrations of three gases are: SO2 = 0.183 M O2 = 0.146 M SO3 = 1.05 M
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol
Using bond energies determine the heat generated when 32 grams of methane, CH4, is burned. (in kJ) CH4 + O2 → CO2 + H2O
1. Based from the thermochemical equation given, O2(9) N2(9) + NO2(9) Calculate the heat associated with the decomposition of 2.75 g of NO2(g) ----> AH = +67.6 kJ Is the reaction exothermic or endothermic?