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How many grams of water will 5 grams of Oxygen produce? 5 grams of Hydrogen? Tonight's Homework: PowerPoint Presentation

How many grams of water will 5 grams of Oxygen produce? 5 grams of Hydrogen? Tonight's Homework:

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How many grams of water will 5 grams of Oxygen produce?

5 grams of Hydrogen?

Tonight's Homework:

Finish Lab Report

pg 259 Numbers 2-10

Lab Report

- Purpose
- Procedure
- Data
- Calculation (mass salt+dish)–(mass dish)
- Results
- Questions/Conclusion

A Word About Mass Conversions

- Calculating the mass-mass conversion between compounds in a chemical reactions is not something that will disappear now that we are moving on

A Word About Mass Conversions

- Calculating the mass-mass conversion between compounds in a chemical reactions is not something that will disappear now that we are moving on
- If you can not calculate conversions from mass-mass, mass –mole , mole-mole…..

A Word About Mass Conversions

- Calculating the mass-mass conversion between compounds in a chemical reactions is not something that will disappear now that we are moving on
- If you can not calculate conversions from mass-mass, mass –mole , mole-mole…..
- You Will Fail

Consider the following reaction2 H2 + O2 2 H2O

Given 24 grams of O2 and 5.0 grams of H2 determine the mass of H2O produced.2 H2 + O2 2 H2O

the mass of H2O produced will be determined by the limiting reactant - do TWO calculations

Two Calculations

- Calculate the amount of product each reactant would produce

Two Calculations

- Calculate the amount of product each reactant would produce
- In this case convert grams of O2 to grams of H2O

Two Calculations

- Calculate the amount of product each reactant would produce
- In this case convert grams of O2 to grams of H2O
- Then convert grams of H2 to grams of H2O

Two Calculations

- Calculate the amount of product each reactant would produce
- In this case convert grams of O2 to grams of H2O
- Then convert grams of H2 to grams of H2O
- Whichever will produce the least amount
of water will be the limiting reactant

calculation for 24 grams of O2

= 27 g of H2O

calculation for 24 grams of O2

= 27 g of H2O

O2 is the LIMITING REACTANT and determines the amount of product

calculation for 5.0 grams of H2

= 45 g of H2O

H2 is the EXCESS REACTANT (some would be left over)

How much hydrogen gas would be left over?

To calculate, first determine how much reacts with all of the oxygen

How much hydrogen gas would be left over?

To calculate, first determine how much reacts with all of the oxygen

given 24 grams of O2

= 3.0 g of H2

3.0 g of H2 reacts so

How much hydrogen gas would be left over?

To calculate, first determine how much reacts with all of the oxygen

given 24 grams of O2

= 3.0 g of H2

3.0 g of H2 reacts so

5.0 g – 3.0 g = 2.0 g of hydrogen remains

Re-Cap

- What steps do you take to convert the mass of one substance to the mass of another in a chemical reaction?

- What steps do you take to determine which substance will be the limiting reactant in a reaction?

Percent Yield 2 AuCl3 +3 Pb 3 PbCl2 + 2 Au

Enoch the Red, an alchemist, wants to try to turn lead into gold (which you can’t do chemically). He finds that mixing lead with an

unidentified compound (gold III chloride) actually produces small amounts of gold. The reaction is as follows:

Percent Yield 2 AuCl3 +3 Pb 3 PbCl2 + 2 Au

Enoch reacts 14.0 g of gold III chloride with excess lead metal. What would be the maximum, THEORETICAL yield of this reaction?

Percent Yield 2 AuCl3 +3 Pb 3 PbCl2 + 2 Au

Enoch reacts 14.0 g of gold III chloride with excess lead metal. What would be the maximum, THEORETICAL yield of this reaction?

Percent Yield 2 AuCl3 +3 Pb 3 PbCl2 + 2 Au

Enoch reacts 14.0 g of gold III chloride with excess lead metal. What would be the maximum, THEORETICAL yield of this reaction?

given 14.0 g of AuCl3

= 9.09 g Au

Percent Yield

Enoch recovers only 1.05 g of gold from the reaction. This could be for many different reasons

some product was lost in the recovery process

the reaction did not go to completion

the AuCl3 is not pure

Percent Yield

the percentage yield expresses the proportion of the expected product that was actually obtained.

Baking Soda Lab

- In the baking soda lab, the formula for the reaction should be :
- NaHCO3+ HCl------> NaCl+ CO2 + H2O
- Balance the equation
- Find the molar masses of
NaHCO3 & NaCl.

- Use the mass from you lab (mass baking soda) to calculate theoretical yield of NaCl

- What do we need to calculate the percent yield now that we have the theoretical yield?

Lab Reports have the theoretical yield?

- The discussion questions were designed to have you calculate a theoretical yield and calculate a percent yield from your actual result.

Finding Limiting Reactant have the theoretical yield?

- Determine the theoretical yield based on the masses of each reactant
- Whichever produces the least amount is your limiting reactant

Finding Theoretical Yield have the theoretical yield?

- Use the mass-mass conversion from the limiting reactant to the desired product
- The product produced by the mass of the limiting reactant is the theoretical yield

Finding Percent Yield have the theoretical yield?

- Use theoretical yield from your mass-mass (gram-gram) calcualtions
- Make sure you have the correct limiting reactant
- Divide the actual yield (given)
by the theoretical yield (from calculation)

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