The ideal gas behavior gets deviated because of the real gases. The particles in the gas occupy finite space and exert interactive forces between themselves.
Explanation:
An ideal gas behavior is at low temperature and at high pressure. According to kinetic theory, the ideal gases "do not occupy space" and there is "no interaction" among the gas molecules. But practically while applying the gas laws this is not the actual case.
<u>Ideal gas equation:
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PV = nRT
The molar mass of NO₂ is 46.0 g/mol
The molar mass of Pb (NO₃)₂ is 331.2 g/mol
First there is a need to find the number of moles of NO₂ via the stoichiometry of reaction:
2Pb(NO₃)₂ → 2PbO (s) + 4NO₂ (g) + 02 (g)
2 × 331.2 g = 4 × 46.0 g
16.87 g = x (mass of NO₂)
mass of NO₂ = 16.87 × 4 × 46 / 2 × 331.2
mass of NO₂ = 3104.08 / 662.4
mass of NO₂ = 4.686 g of NO₂
Now the number of moles are:
1 mole NO₂ = 46.0 g
x moles of NO₂ = 4.686 g
4.686 × 1 / 46.0 = 0.101 moles of NO₂
1 mole = 22.4 L (at STP)
0.101 moles of NO₂ = 0.101 × 22.4 / 1
= 2.26 L
To answer this, we look at the polarities of these molecules given. A molecule is said to be polar when there is an unequal shraing of electrons the opposite is called nonpolar.
CH4 = nonpolar
CH3OH = polar
CH3 CH3 = nonpolar
CH3 CH2 CH2 OH = polar
<span>CH3 CH2 CH2 CH2 CH2 CH3 = nonpolar</span>