Explanation:
(a) The molecular equations shows the equation in which all the species of the reactants and the products are in molecules and the net charge is zero.
The complete ionic equations shows the equation in which all the species of the reactants and the products are in dissociated form and are represented as ions.
The net ionic equations shows the equation in which all the species of the reactants and the products are in dissociated form and do not show the spectator ions which are same in the reactants and the products.
(b) If there is no spectator ions in the reaction, then the complete and the net ionic equations would be identical.
Explanation:
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Benzene reacts with O₂ to produce CO₂ and H₂O, i.e.
C₆H₆ + 7.5 O₂ → 6 CO₂ + 3 H₂O
According to equation,
78.11 g (1 mole) C₆H₆ reacts to produce = 264 g (6 moles) of CO₂
Hence,
7.80 g C₆H₆ when reacted will produce = X g of CO₂
Solving for X,
X = (7.80 g × 264 g) ÷ 78.11 g
X = 26.36 g of CO₂
Theoretical Yield:
26.36 g of CO₂ produced is theoretical yield which shows 100% reaction between benzene and oxygen.
Actual Yield:
According to statement the actual amount of CO₂ produced is 3.0 g of CO₂.
%age Yield:
%age Yield = (Actual Yield ÷ Theoretical Yield) × 100
Putting Values,
%age Yield = (3.00 g ÷ 26.36 g) × 100
%age Yield = 11.38 %
Because you need oxygen in your blood stream and it revives cells as it travels through.
3.3 g of SO₂ is a larger quantity in moles.
<h3>
What is moles?</h3>
Mole, also spelled mol, in chemistry, a standard scientific unit for measuring large quantities of very small entities such as atoms, molecules, or other specified particles.
The mole designates an extremely large number of units, 6.02214076 × 
. The General Conference on Weights and Measures defined the mole as this number for the International System of Units (SI) effective from May 20, 2019. The mole was previously defined as the number of atoms determined experimentally to be found in 12 grams of carbon-12.
The number of units in a mole also bears the name Avogadro’s number, or Avogadro’s constant, in honour of the Italian physicist Amedeo Avogadro (1776–1856). Avogadro proposed that equal volumes of gases under the same conditions contain the same number of molecules, a hypothesis that proved useful in determining atomic and molecular weights and which led to the concept of the mole.
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