Changes

===About Yield===

: The experimental '''yield''' from a [[Chemical Reaction|chemical reaction]] is often not as large as the theoretical '''yield''' because not all of the [[reactant]]s will [[Chemical Reaction|react]]. This experimental '''yield''' is often expressed as a [[percentage]] of the theoretical '''yield''' and is known as the [[Percentage Yield]].

===Examples===

{| class="wikitable"

Calculate the '''yield''' of [[Magnesium Oxide]] given 48g of [[Magnesium]] and excess [[Oxygen]].

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'''Write the Balanced Symbol Equation'''

2Mg + O₂ → 2MgO

'''Write the Balanced Symbol Equation'''

CH₄ + 2O₂ → 2H₂O + CO₂

'''Write the Balanced Symbol Equation'''

NaOH + HCl → NaCl + H₂O

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M_r of CH₄ = 16g

M_r of NaOH = 40g

M_r of NaCl = 58.5g

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2 [[mole]]s of Mg are needed for every 2 [[mole]]s of MgO

1 [[mole]] of HCl and NaOH are needed for every 1 [[mole]] of NaCl

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No. [[Mole]]s = <math>\frac{Mass}{M_r}</math>

No. [[Mole]]s = <math>\frac{48}{24}</math>

No. [[Mole]]s = <math>\frac{Mass}{M_r}</math>

No. [[Mole]]s = <math>\frac{Mass}{M_r}</math>

|}