The equation of state for a hypothetical ideal gas is known as the ideal gas law, sometimes known as the general gas equation. i.e. PV = nRT or P1V1 = P2V2.
- According to the ideal gas law, the sum of the absolute temperature of the gas and the universal gas constant is equal to the product of the pressure and volume of one gram of an ideal gas.
- Robert Boyle, Gay-Lussac, and Amedeo Avogadro's observational work served as the basis for the ideal gas law. The Ideal gas equation, which simultaneously describes every relationship, is obtained by combining all of their observations into a single statement.
- When applying the gas constant R = 0.082 L.atm/K.mol, pressure, volume, and temperature should all be expressed in units of atmospheres (atm), litres (L), and kelvin (K).
- At high pressure and low temperature, the ideal gas law basically fails because molecule size and intermolecular forces are no longer negligible but rather become significant considerations.
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Answer:
There are produced 6.72 g
Explanation:
This is the reaction:
C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O
1 mol of glucose reacts with 6 moles of oxygen, to make 6 moles of dioxide and 6 moles of water
Molar mass of CO₂ = 46 g/m
Moles CO₂ = 10.3 g/ 46g/m = 0.224 moles
Ratio is 6:1
6 moles of CO₂ are made from 1 mol of glucose
0.224 moles of CO₂ are made from (0.224 . 1)/6 = 0.0373 moles of glucose
Molar mass glucose = 180.15 g/m
Mass glucose = moles . molar mass
0.0373 m . 180.15 g/m = 6.72 g