ORG-14

Percent yield

Y = 100 m_actual / m_theoretical.

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StoichiometryYield

Governing equation

Y=100\,m_{\mathrm{act}}/m_{\mathrm{th}}

where

m_{act}: Actual mass (g)
m_{th}: Theoretical mass (g)
Y: Yield (%)

Lecture brief

Historical brief

Hammett (1937) and Taft linear free-energy, E-factor green metrics, Woodward–Fieser UV and Claisen equilibria are how organic chemistry became predictive. The lab is substituent, waste and tautomer. This sheet (ORG-14 — Percent yield) is the form associated with Yield. Working symbols: $m_{act}$ , $m_{th}$ $\rightarrow$ $Y$ . The theoretical mass is the limiting-reagent mass times the stoichiometric ratio.

Purpose

Purpose: compute

Y

from

m_{act}

m_{th}

in Organic chemistry via

Y=100\,m_{\mathrm{act}}/m_{\mathrm{th}}

Y = 100 m_actual / m_theoretical. Use it when a real organic chemistry question must be answered in SI before a code check.

Live realistic example

In symbols

Live case. Given

m_{act} = 8.400\,\mathrm{g}

m_{th} = 12.000\,\mathrm{g}

, the governing relation

Y=100\,m_{\mathrm{act}}/m_{\mathrm{th}}

yields

Y = 70.0\,\mathrm{%}

. Isolated product vs calculated theoretical mass. Move a slider: the numbers are this situation, not a canned story.

Calculator

Inputs

Actual mass m_{act}8.4 gTheoretical mass m_{th}12 g

Outputs

Yield Y70.0 %

Reading speed

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Narration of this film

Isolated product vs calculated theoretical mass.

The theoretical mass is the limiting-reagent mass times the stoichiometric ratio.

Reading speed

Watch on YouTube