The metabolic oxidation of glucose, C, H1206, in our bodies produces CO2, which is expelled from our lungs as a gas: Part A C,H12O6 (aq) + 602(9) → 6CO2(g) + 6H2O(1) Calculate the volume of dry CO2 produced at body temperature (37 °C) and 0.950 atm when 23.5 g of glucose is consumed in this reaction. Express your answer using three significant figures. V = L Submit Request Answer Part B Calculate the volume of oxygen you would need, at 1.00 atm and 298 K, to completely oxidize 51 g of glucose. Express your answer using three significant figures. ? V= L

The metabolic oxidation of glucose, C, H1206, in our bodies produces CO2, which is expelled from our lungs as a gas: Part A C,H12O6 (aq) + 602(9) → 6CO2(g) + 6H2O(1) Calculate the volume of dry CO2 produced at body temperature (37 °C) and 0.950 atm when 23.5 g of glucose is consumed in this reaction. Express your answer using three significant figures. V = L Submit Request Answer Part B Calculate the volume of oxygen you would need, at 1.00 atm and 298 K, to completely oxidize 51 g of glucose. Express your answer using three significant figures. ? V= L

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 combustion of fuel in your car engine requires oxygen gas, which is supplied as air (21% oxygen molecules) into the engine. Consider a car that is using 100% ethanol, C2H5OH, as fuel. If your engine intakes 2.71 L of air per minute at 1.00 atm and 25ºC, what is the maximum volume of ethanol (0.789 g/mL) that can be burned per minute? Hint: You can ignore the "per minute" information because both the ethanol and air are being quantified per minute. Enter the answer to three significant figures in units of mL.
The metabolic oxidation of glucose, C6H12O6, in our bodies produces CO2, which is expelled from our lungs as a gas: C6H12O6(aq) + 6O2(g) → 6CO2(g) + 6H2O(l) Calculate the volume of dry CO2 produced at body temperature (37 °C) and 0.970 atm when 23.7 g of glucose are consumed in this reactions.
Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq) + 6H2O(1)-2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 759 mm Hg. If the wet H, mol. The vapor gas formed occupies a volume of 7.78 L, the number of moles of Al reacted was pressure of water is 23.8 mm Hg at 25 °C.
Please help me to give you thumbs up
Oxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KC103 (8) 2KCl(s) + 302(g) The product gas, O2, is collected over water at a temperature of 20 °C and a pressure of 757.0 mm Hg. If the wet O₂ gas formed occupies a volume of 5.22 L, the number of moles of KCIO, reacted was 5.3 mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
What volume of carbon dioxide will 3.26 g of antacid made of calcium carbonate produce at 37.0 °C and 1.00 atm in the stomach according to the following reaction? CaCO3 (s) + 2 HCI (aq) → CaCl2 (aq) + H2O (1) + CO2 (g)
What is the pressure of the air, in atmatm, in the lungs when the gas expands to 150.0 mLmL at a body temperature of 37 ∘C∘C, and the amount of gas remains constant?
Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NaOH(aq) + 6H₂O2NaAl(OH),(aq) + 3H₂(g) In an experiment, the H₂ gas is collected over water in a vessel where the total pressure is 751 torr and the temperature is 25°C, at which temperature the vapor pressure of water is torr. If the wet H₂ gas formed occupies a volume of 7.02 L, the number of moles of H₂ 23.8 ton. Under these conditions, the partial pressure of H, is formed is mol.
Gaseous iodine pentafluoride, IFs, can be prepared by the reaction of solid iodine and gaseous fluorine: 2(s) + 5F:(g) → 2IF:(g) A 10.00 L flask is charged with 11.0 grams of l2 and 2.00 atm of F2 at 25°C. The flask is heated to 100°C until one of the reagents is completely consumed. What will be the total pressure (in atm) of the final products in the flask at 100°C? (Assume ideal gas behavior).
Consider the following reaction:2 ��(�) + ��2 (�) → ��2��3 (�) + �2�(�)What volume of CO2 (g) at 22.3°C and 1.25 atm is needed to react completely with 1.00 g of LiOH? Express your answer in litres
Find the volume in liters of hydrogen gas produced at 0.959 atm and 298 K from the reaction of 30.4 g of metallic iron with excess HCl(aq) according to the reaction: 2 Fe(s) + 6 HCl(aq) → 2 FeCl3(aq) + 3 H2(g)
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.