Difference between revisions of "Yield (Chemistry)"
(→Examples) |
(→Examples) |
||
| Line 30: | Line 30: | ||
|- | |- | ||
| style="height:20px; width:200px; text-align:left;" | | | style="height:20px; width:200px; text-align:left;" | | ||
| − | Find the [[Relative Formula Mass]] of the [[reactant]]s and [[product]] | + | Find the [[Relative Formula Mass]] of the relevant [[reactant]]s and [[product]]. |
| − | |||
| − | |||
M<sub>r</sub> of 2Mg = 48g | M<sub>r</sub> of 2Mg = 48g | ||
| − | M<sub>r</sub> of | + | M<sub>r</sub> of 2MgO = 80g |
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| style="height:20px; width:200px; text-align:left;" | | | style="height:20px; width:200px; text-align:left;" | | ||
| − | Find the [[Relative Formula Mass]] of the [[reactant]]s and [[product]] | + | Find the [[Relative Formula Mass]] of the relevant [[reactant]]s and [[product]]. |
| − | |||
| − | |||
M<sub>r</sub> of CH<sub>4</sub> = 16g | M<sub>r</sub> of CH<sub>4</sub> = 16g | ||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
M<sub>r</sub> of CO<sub>2</sub> = 44g | M<sub>r</sub> of CO<sub>2</sub> = 44g | ||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| − | |||
| style="height:20px; width:200px; text-align:left;" | | | style="height:20px; width:200px; text-align:left;" | | ||
| − | Find the [[Relative Formula Mass]] of the [[reactant]]s and [[product]] | + | Find the [[Relative Formula Mass]] of the relevant [[reactant]]s and [[product]]. |
M<sub>r</sub> of NaOH = 40g | M<sub>r</sub> of NaOH = 40g | ||
M<sub>r</sub> of HCl = 36.5g | M<sub>r</sub> of HCl = 36.5g | ||
| − | |||
| − | |||
M<sub>r</sub> of NaCl = 58.5g | M<sub>r</sub> of NaCl = 58.5g | ||
| − | |||
| − | |||
| − | |||
| − | |||
|- | |- | ||
| style="height:20px; width:200px; text-align:left;" | | | style="height:20px; width:200px; text-align:left;" | | ||
State the [[ratio]] of [[mole]]s of each [[chemical]] needed. | State the [[ratio]] of [[mole]]s of each [[chemical]] needed. | ||
| − | 2 [[mole]]s of Mg are needed for every | + | 2 [[mole]]s of Mg are needed for every 2 [[mole]]s of MgO |
| style="height:20px; width:200px; text-align:left;" | | | style="height:20px; width:200px; text-align:left;" | | ||
State the [[ratio]] of [[mole]]s of each [[chemical]] needed. | State the [[ratio]] of [[mole]]s of each [[chemical]] needed. | ||
| − | 1 [[mole]] of CH<sub>4</sub> is needed for every | + | 1 [[mole]] of CH<sub>4</sub> is needed for every 1 [[mole]] of CO<sub>2</sub> |
| style="height:20px; width:200px; text-align:left;" | | | style="height:20px; width:200px; text-align:left;" | | ||
State the [[ratio]] of [[mole]]s of each [[chemical]] needed. | State the [[ratio]] of [[mole]]s of each [[chemical]] needed. | ||
| − | 1 [[mole]] of HCl are needed for every 1 [[mole]] of | + | 1 [[mole]] of HCl and NaOH are needed for every 1 [[mole]] of NaCl |
|- | |- | ||
Revision as of 17:12, 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. |
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 relevant reactants and product. Mr of 2Mg = 48g Mr of 2MgO = 80g |
Find the Relative Formula Mass of the relevant reactants and product. Mr of CH4 = 16g Mr of CO2 = 44g |
Find the Relative Formula Mass of the relevant reactants and product. Mr of NaOH = 40g Mr of HCl = 36.5g Mr of NaCl = 58.5g |
|
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 |