The following unbalanced equation illustrates the over reaction by which the body utilizes glucose to produce energy.
C6H12O6(s) + O2(g) --> CO2(g) + H2O(l)
What is the conversion factor that allows for the calculation of moles of carbon dioxide based on moles of glucose
The following unbalanced equation illustrates the over reaction by which the body utilizes glucose to produce...
The human body converts glucose (C6H12O6) to carbon dioxide and water. The balanced chemical equation for the reaction is: C6H12O6 + 6 O2 → 6 CO2 + 6 H2O If you ate a candy bar that contained 22.2 g of glucose (C6H12O6), how many grams of water will the body produce from the glucose you ate? How many grams of CO2 would that make?
1. In the reaction between glucose and oxygen below, how many grams of glucose is required to produce 12.2 L of carbon dioxide if the density of Carbon dioxide is 1.26 g/L, C2H5OH, is 0.789g/mL. C6H12O6(s) + 6 O2(g) = 6 CO2(g) +6 H2O 2. When 10.6 g of boron trichloride is reacted with water, 5.12 g of Hydrochloric acid is produced. Using the following balanced equation, calculate the percent yield for HCl for the reaction? (BCl3 = 117.17 g/mol,...
Glucose, C6H12O6, is used as an energy source by the human body. The overall reaction in the body is described by the equationC6H12O6(aq) + 6O2(g) — 6CO2(g) + 6H2O(1) Calculate the number of grams of oxygen required to convert 38.0 g of glucose to CO2, and H2O. mass of O2 = _______ g Calculate the number of grams of CO2, produced. mass of CO2 = _______ g
question 5, 6 5. (10 pts) Helena compares oxidation with reduction. Match each term with the correct definition a) Oxidation • Gain of oxygen • Gain of hydrogen b) Reduction • Loss of electron • Decrease in oxidation number • Gain of electron 6. Jasmine finds that the carbohydrate is one of the major sources of energy of our body. The combustion of the carbohydrate glucose produces carbon dioxide and water: C6H12O6 + O2 CO2 + H2O (unbalanced) a) (2...
Consider the following unbalanced equation: O2(g) + C4H10(g) → CO2(g) + H2O(l) If 3.56×102 moles of O2(g) and 47.3 moles of C4H10(g) are allowed to react to produce 1.10×102 moles of CO2(g), what is the percent yield of the reaction? 29.2% 58.1% 89.5% 89.9% 65.7%
2. Given the unbalanced equation: C3H8 + O2 CO2 + H2O a. How many moles of oxygen gas are required to make 4.00 moles of carbon dioxide? b. How many moles of C3H8 must be used to produce 2.00 grams of water?
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol ______kJ/mol
What mass of ethene (C2H4) must burn to produce 46.4 g of carbon dioxide? The UNBALANCED equation is shown below: C2H4 + O2 → CO2 + H2O
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, Δ H o f CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol
8. When glucose reacts with oxygen in living systems, carbon dioxide and water are produced, and a great deal of energy is liberated. C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O(g) What weight of carbon dioxide can be produced from the reaction of 10.0 grams of glucose with 10.0 grams of oxygen? (a) 2.29 g (b) 2.44 g (c) 13.8 g (d) 14.7 g (e) none of these 9.Based on the balanced chemical equation shown below, determine the...