Answer:
B. It moves more rapidly in the same direction.
Explanation:
Option B
dumbbell is the shape of 3p atomic orbital
<u>Explanation:</u>
Atomic orbitals are three-dimensional places inside an atom where there is a tremendous chance of detecting electrons. The p orbital, which develops in complexity and ought 2 spaces encompassing the atom core, or is defined as possessing a dumbbell pattern. The 3p atomic orbital is at energy level 3, as seen by the number 3 filed ere the character.
These orbitals have identical appearances but are arranged asymmetrically in location. p orbitals are wavefunctions with l=1. They ought an angular frequency that is ununiform at each angle. They have an appearance that is much defined as a "dumbbell".
Answer:
68.1% is percent yield of the reaction
Explanation:
The reaction of methane with oxygen is:
CH₄ + 2O₂ → CO₂ + 2H₂O
<em>Where 2 moles of oxygen react per mole of CH₄</em>
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Percent yield is:
Actual yield (28.2g CO₂) / Theoretical yield * 100
To solve this question we need to find theoretical yield finding limiting reactant :
<em>Moles CH₄:</em>
15.1g CH₄ * (1mol / 16.04g) = 0.9414 moles
<em>Moles O₂:</em>
81.2g * (1mol / 32g) = 2.54 moles
For a complete reaction of 0.9414 moles of CH₄ are needed:
0.9414 moles CH₄ * (2 mol O₂ / 1mol CH₄) = 1.88 moles of O₂. As there are 2.54 moles, O₂ is in excess and <em>CH₄ is limiting reactant</em>
In theoretical yield, the moles of methane added = Moles of CO₂ produced. That is 0.9414 moles CO₂. In grams = Theoretical yield:
0.9414 moles CO₂ * (44.01g / mol) = 41.43g CO₂
Percent yield: 28.2g CO₂ / 41.43g CO₂ * 100=
<h3>68.1% is percent yield of the reaction</h3>
