Theoretical, Actual, and Percent Yield Problems Example 1.

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Presentation transcript:

Theoretical, Actual, and Percent Yield Problems Example 1

First we’ll review some important definitions.

Yield–

First we’ll review some important definitions. Yield–Simply means the amount of a particular product formed in a chemical reaction

Theoretical Yield

–(also called predicted yield)

Theoretical Yield –(also called predicted yield) is the amount of product predicted by a stoichiometric calculation.

In other words, if we’re given the amounts of reactants and asked to use stoichiometry to find the mass of a product, then we are finding the theoretical (or predicted ) yield of that product.

For various reasons, when a reaction is carried out in a real physical setting, like a lab or an industrial site, we don’t always get the amount of a product predicted.

Actual yield

For various reasons, when a reaction is carried out in a real physical setting, like a lab or an industrial site, we don’t always get the amount of a product predicted. Actual yield – the amount of a product that is actually obtained in a reaction.

Percent Yield

– the formula we use for percent yield is:

Percent Yield – the formula we use for percent yield is:

Percent Yield – the formula we use for percent yield is:

Percent Yield – the formula we use for percent yield is:

Percent Yield – the formula we use for percent yield is:

Percent Yield – the formula we use for percent yield is:

If the actual yield of a particular product was equal to the theoretical, or predicted yield,

If the actual yield of a particular product was equal to the theoretical, or predicted yield, then the percent yield would be 100%.

In many reactions that take place in labs and industrial sites, the actual yield is less than the theoretical, or predicted yield.

In these cases, the percent yield is less than 100%.

Example Problem

Given the equation:

Example Problem Given the equation:

Example Problem Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced.

Example Problem Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced.

Example Problem Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Example Problem Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg? b)What is the actual yield of NH 3 ?

Example Problem Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg? b)What is the actual yield of NH 3 ? c)What is the percent yield of NH 3 ?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2 Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2 Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2 Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2 Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3 Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg? kg H 2  g H 2  mol H 2  mol NH 3  g NH 3 Plan:

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 Plan: a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. kg H 2  g H 2  mol H 2  mol NH 3  g NH 3  kg NH 3 a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg?

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. a)What is the theoretical yield of NH 3 in kg? Theoretical yield = kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. b)What is the actual yield of NH 3 ? Theoretical yield = kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. b)What is the actual yield of NH 3 ? Theoretical yield = kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. b)What is the actual yield of NH 3 ? Theoretical yield = kg The actual yield of NH 3 is 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. b)What is the actual yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg The actual yield of NH 3 is 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. c)What is the percent yield of NH 3 ? Theoretical yield = kg Actual yield = 4.92 kg % yield = 35.0%

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. Theoretical yield = kg Actual yield = 4.92 kg % yield = 35.0% a)The theoretical yield is kg b)The actual yield is 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. Theoretical yield = kg Actual yield = 4.92 kg % yield = 35.0% a)The theoretical yield is 14.1 kg b)The actual yield is 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. Theoretical yield = kg Actual yield = 4.92 kg % yield = 35.0% a)The theoretical yield is 14.1 kg b)The actual yield is 4.92 kg

Given the equation: When 2.50 kg of H 2(g) is added to an excess of N 2(g) at 450°C, 4.92 kg of NH 3(g) is produced. Theoretical yield = kg Actual yield = 4.92 kg % yield = 35.0% a)The theoretical yield is 14.1 kg b)The actual yield is 4.92 kg c)The percent yield is 35.0%