Answer :
Final Answer:
1. The volume of dry CO2 produced at body temperature (37 °C) and 99.3 kPa when 25.5 g of glucose is consumed in this reaction is approximately 11.6 L.
2. To calculate the volume of dry CO2 produced, we can use the ideal gas law, which relates the number of moles of a gas to its volume, temperature, and pressure. First, we need to find the moles of glucose consumed.
Explination:
Given:
- Mass of glucose (C6H12O6) = 25.5 g
- Molar mass of glucose (C6H12O6) = 180.16 g/mol
Using the formula: Moles = Mass / Molar mass
Moles of glucose = 25.5 g / 180.16 g/mol ≈ 0.1413 moles
Now, we can use the balanced chemical equation to determine the moles of CO2 produced. From the equation, we see that 1 mole of glucose produces 6 moles of CO2.
Moles of CO2 produced = 0.1413 moles glucose * 6 moles CO2/mole glucose ≈ 0.8478 moles CO2
Now, we can apply the ideal gas law:
PV = nRT
Where:
P = pressure (99.3 kPa)
V = volume (which we need to find)
n = moles of CO2 (0.8478 moles)
R = ideal gas constant (8.314 J/(mol*K))
T = temperature in Kelvin (37 °C = 310 K)
Now, solve for V:
V = (nRT) / P
V = (0.8478 moles * 8.314 J/(mol*K) * 310 K) / 99.3 kPa * 1000 Pa/kPa
V ≈ 11.6 L (rounded to three significant figures)
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Final answer:
To calculate the volume of CO2 produced and the volume of oxygen needed in the metabolic oxidation of glucose, use the ideal gas law equation.
Explanation:
To calculate the volume of dry CO2 produced at body temperature and 99.3kPa when 25.5 g of glucose is consumed, we need to use the ideal gas law equation: PV = nRT. First, convert the mass of glucose to moles by dividing it by the molar mass of glucose. Then, use the balanced equation to determine the mole ratio between glucose and CO2. Finally, use the ideal gas law equation to calculate the volume of CO2. For part B, follow the same steps using the molar mass of glucose to convert the mass to moles, and then calculate the volume of oxygen using the ideal gas law equation.
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