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Difference between revisions of "Yield (Chemistry)"

(Created page with "==Key Stage 4== ===Meaning=== Yield is the mass of product in a chemical reaction. ===About Yield===")
 
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==Key Stage 4==
 
==Key Stage 4==
 
===Meaning===
 
===Meaning===
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[[Yield]] is the [[mass]] of [[product]] in a [[Chemical Reaction|chemical reaction]].
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'''Yield''' is the [[mass]] of [[product]] in a [[Chemical Reaction|chemical reaction]].
  
 
===About Yield===
 
===About Yield===
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: The theoretical '''yield''' of [[product]] form a [[Chemical Reaction|chemical reaction]] can be calculated using the [[Balanced Symbol Equation|balanced symbol equation]] and the [[Relative Formula Mass|relative formula masses]] of all the [[molecule]]s involved.
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: 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]].
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===Examples===
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{| class="wikitable"
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| style="height:20px; width:200px; text-align:center;" |
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Calculate the '''yield''' of [[Magnesium Oxide]] given 48g of [[Magnesium]] and excess [[Oxygen]].| style="height:20px; width:200px; text-align:center;" |
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Find the '''yield''' of [[Carbon Dioxide]] when 32g of [[Methane]] [[Chemical reaction|reacts]] with excess [[Oxygen]].
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| style="height:20px; width:200px; text-align:center;" |
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Find the '''yield''' of [[Sodium Chloride]] when 80g of [[Sodium Hydroxide]] [[Chemical Reaction|react]] with 73g of [[Hydrochloric Acid]].
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|-
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| style="height:20px; width:200px; text-align:left;" |
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'''Write the Balanced Symbol Equation'''
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2Mg + O<sub>2</sub> → 2MgO
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| style="height:20px; width:200px; text-align:center;" |
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'''Write the Balanced Symbol Equation'''
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CH<sub>4</sub> + 2O<sub>2</sub> → 2H<sub>2</sub>O + CO<sub>2</sub>
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| style="height:20px; width:200px; text-align:left;" |
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'''Write the Balanced Symbol Equation'''
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NaOH + HCl → NaCl + H<sub>2</sub>O
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|-
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| style="height:20px; width:200px; text-align:left;" |
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Find the [[Relative Formula Mass]] of the [[reactant]]s and [[product]]s.
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M<sub>r</sub> of Mg = 24g
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M<sub>r</sub> of 2Mg = 48g
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M<sub>r</sub> of O<sub>2</sub> = 16x2
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M<sub>r</sub> of O<sub>2</sub> = 32g
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M<sub>r</sub> of MgO = 24+16
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M<sub>r</sub> of MgO = 40g
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| style="height:20px; width:200px; text-align:left;" |
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Find the [[Relative Formula Mass]] of the [[reactant]]s and [[product]]s.
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M<sub>r</sub> of CH<sub>4</sub> = 12+1x4
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M<sub>r</sub> of CH<sub>4</sub> = 16g
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M<sub>r</sub> of O<sub>2</sub> = 16x2
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M<sub>r</sub> of O<sub>2</sub> = 32g
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M<sub>r</sub> of 2O<sub>2</sub> = 64g
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M<sub>r</sub> of CO<sub>2</sub> = 12+16x2
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M<sub>r</sub> of CO<sub>2</sub> = 44g
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M<sub>r</sub> of H<sub>2</sub>O = 1x2+16
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M<sub>r</sub> of H<sub>2</sub>O = 18
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M<sub>r</sub> of 2H<sub>2</sub>O = 36g
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| style="height:20px; width:200px; text-align:left;" |
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Find the [[Relative Formula Mass]] of the [[reactant]]s and [[product]]s.
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M<sub>r</sub> of NaOH = 40g
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M<sub>r</sub> of HCl = 36.5g
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M<sub>r</sub> of NaCl = 23+35.5
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M<sub>r</sub> of NaCl = 58.5g
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M<sub>r</sub> of H<sub>2</sub>O = 1x2+16
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M<sub>r</sub> of H<sub>2</sub>O = 18
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|-
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| style="height:20px; width:200px; text-align:left;" |
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State the [[ratio]] of [[mole]]s of each [[chemical]] needed.
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2 [[mole]]s of Mg are needed for every 1 [[mole]] of O<sub>2</sub>
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| style="height:20px; width:200px; text-align:left;" |
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State the [[ratio]] of [[mole]]s of each [[chemical]] needed.
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1 [[mole]] of CH<sub>4</sub> is needed for every 2 [[mole]]s of O<sub>2</sub>
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| style="height:20px; width:200px; text-align:left;" |
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State the [[ratio]] of [[mole]]s of each [[chemical]] needed.
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1 [[mole]] of HCl are needed for every 1 [[mole]] of NaOH
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|-
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| style="height:20px; width:200px; text-align:left;" |
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Find the number of [[mole]]s supplied of the known [[mass]].
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No. [[Mole]]s = <math>\frac{Mass}{M_r}</math>
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No. [[Mole]]s = <math>\frac{48}{24}</math>
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No. [[Mole]]s = 2 Mole
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Therefore 1 [[mole]] of O<sub>2</sub> is needed.
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1 [[mole]] of O<sub>2</sub> = 32g
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| style="height:20px; width:200px; text-align:left;" |
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Find the number of [[mole]]s supplied of the known [[mass]].
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No. [[Mole]]s = <math>\frac{Mass}{M_r}</math>
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No. [[Mole]]s = <math>\frac{32}{16}</math>
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No. [[Mole]]s = 2 Mole
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Therefore 4 [[mole]]s of O<sub>2</sub> are needed.
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4 [[mole]]s of O<sub>2</sub> = 128g
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| style="height:20px; width:200px; text-align:left;" |
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Find the number of [[mole]]s supplied of the known [[mass]].
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No. [[Mole]]s = <math>\frac{Mass}{M_r}</math>
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No. [[Mole]]s = <math>\frac{20}{40}</math>
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No. [[Mole]]s = 0.5 Mole
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Therefore 0.5 [[mole]] of HCl is needed.
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0.5 [[mole]] of HCl = 18.25g
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 +
|}

Revision as of 16:48, 12 January 2019

Key Stage 4

Meaning

Yield is the mass of product in a chemical reaction.

About Yield

The theoretical yield of product form a chemical reaction can be calculated using the balanced symbol equation and the relative formula masses of all the molecules involved.
The experimental yield from a chemical reaction is often not as large as the theoretical yield because not all of the reactants will react. This experimental yield is often expressed as a percentage of the theoretical yield and is known as the Percentage Yield.

Examples

Calculate the yield of Magnesium Oxide given 48g of Magnesium and excess Oxygen.| style="height:20px; width:200px; text-align:center;" | Find the yield of Carbon Dioxide when 32g of Methane reacts with excess Oxygen.

Find the yield of Sodium Chloride when 80g of Sodium Hydroxide react with 73g of Hydrochloric Acid.

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

Find the Relative Formula Mass of the reactants and products.

Mr of Mg = 24g

Mr of 2Mg = 48g

Mr of O2 = 16x2

Mr of O2 = 32g

Mr of MgO = 24+16

Mr of MgO = 40g

Find the Relative Formula Mass of the reactants and products.

Mr of CH4 = 12+1x4

Mr of CH4 = 16g

Mr of O2 = 16x2

Mr of O2 = 32g

Mr of 2O2 = 64g

Mr of CO2 = 12+16x2

Mr of CO2 = 44g

Mr of H2O = 1x2+16

Mr of H2O = 18

Mr of 2H2O = 36g

Find the Relative Formula Mass of the reactants and products.

Mr of NaOH = 40g

Mr of HCl = 36.5g

Mr of NaCl = 23+35.5

Mr of NaCl = 58.5g

Mr of H2O = 1x2+16

Mr of H2O = 18

State the ratio of moles of each chemical needed.

2 moles of Mg are needed for every 1 mole of O2

State the ratio of moles of each chemical needed.

1 mole of CH4 is needed for every 2 moles of O2

State the ratio of moles of each chemical needed.

1 mole of HCl are needed for every 1 mole of NaOH

Find the number of moles supplied of the known mass.

No. Moles = \(\frac{Mass}{M_r}\)

No. Moles = \(\frac{48}{24}\)

No. Moles = 2 Mole

Therefore 1 mole of O2 is needed.

1 mole of O2 = 32g

Find the number of moles supplied of the known mass.

No. Moles = \(\frac{Mass}{M_r}\)

No. Moles = \(\frac{32}{16}\)

No. Moles = 2 Mole

Therefore 4 moles of O2 are needed.

4 moles of O2 = 128g

Find the number of moles supplied of the known mass.

No. Moles = \(\frac{Mass}{M_r}\)

No. Moles = \(\frac{20}{40}\)

No. Moles = 0.5 Mole

Therefore 0.5 mole of HCl is needed.

0.5 mole of HCl = 18.25g

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