Lab 1 determination of the empirical formula of silver oxide

What is the percent composition of silver and oxygen in silver oxide? The percent yield reflects the actual amount of product formed versus the maximum that might have been obtained.

What is the empirical formula of silver oxide? We also used a different ring stand as it was a tripod stand and therefore could account for the heat reaching it improperly, although since the other two trials went better, and the other teams were utilizing a similar tripod stand, I doubt it would be the case.

The reason for this is that we all immediately noticed that the reactant we have put in was dark and smooth dust and the product that was produced was the opposite entirely. This shows that the empirical formula is affected by the smallest change in mass and needs to be calculated with great precision and accuracy.

Write a balanced chemical equation for the decomposition of silver oxide to form silver metal and oxygen. Due to the above mentioned experimental error, I would have to say that my confidence level on a scale of about my conclusion would be about an 8. Use the molar masses of silver and oxygen to calculate the number of moles of each product.

Many small mistakes could have happened during the experiment. Applications Discussion All though the empirical formula differed in each trial, the percent yield was not drastic.

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What is the empirical formula of silver oxide? Use the molar masses of silver and oxygen to calculate the number of moles of each product. Calculate the mass of silver oxide and the mass of the silver metal product. Calculate the molar mass of silver oxide.

Calculate the theoretical yield of silver metal in this experiment.

Determination of the Empirical Formula of Silver Oxide—AP* Chemistry Classic Laboratory Kit

Enter the answers in your Data Results Table. One of the major mistakes we made was that when we switched the burner that was running out with the one that was full, the new burner was not working properly so for safety we had to turn it off an switch it with one that did.

While conducting the experiment, every team noticed that our descriptions of the product were in the same words: Use the law of conservation of mass to calculate the mass of oxygen produced with the silver. I would give my confidence in our data an eight. Calculate the ratio between the number of moles of silver and the number of moles of oxygen in the product.

Enter the answers in the Data Results table. It would also be interesting to try such an experiment with other kinds of metals to see what changes we can observe in the substance after heating. Calculate the molar mass of silver oxide. This means that for a couple of seconds at least the silver oxide stopped being heated, which could have delayed the burning process and affected the amount of silver oxide left over.

Write a balanced chemical equation for the decomposition of silver oxide to form silver metal and oxygen. Calculate the ratio between the number of moles of silver and the number of moles of oxygen in the product. In the future it would be interesting to conduct the experiment at least one more time ourselves so as to figure out if our altered numbers in our results were caused by this experimental error or something else we did wrong and did not notice.

Use the following equation to calculate the percent yield of silver metal produced in this experiment. Calculate the mass of silver oxide and the mass of the silver metal product. Calculate the theoretical yield of silver metal in this experiment.

My group was the first group that is described in my results, referred to in the data tables as Trial 1. Use the law of conservation of mass to calculate the mass of oxygen that combined with the silver.

Photos of My Work: Use the following equation to calculate the percent yield of silver metal produced in this experiment. The difference in this case means that we had a bit too much silver metal left over, and my hypothesis is that it would be because we had a small incident while doing the experiment.

What is the percent composition of silver and oxygen in silver oxide?Oct 26,  · The lab was to determine the empirical formula of a silver oxide.?

i recorded a mass of the crucible and lid as g. the mass of the crucible & lid with the silver oxide was g. The mass of the crucible & lid and the silver Status: Resolved.

The ratio between silver and oxygen is about 5 to 3. Therefore the empirical formula is Ag 5 O 3. 5. The balanced equation for the decomposition of silver oxide to form silver metal and oxygen is 2Ag 5 O 3 10Ag + 3O 2 6.

The calculations show the empirical formula of Ag2O, Each trial proved an Ag to O ratio of 2 to 1 which is used to write the empirical formula. An empirical formula describes the composition of a compound in terms of the simplest whole number ratio. Lab 2 - Determination of the Empirical Formula of Magnesium Oxide Goal and Overview The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal.

Calculate the empirical formula for silver oxide based on your lab data. Show your work. Calculate the percent composition of silver in one mole of silver oxide using your empirical formula. This is the theoretical percent composition.

Calculate the percent composition of silver in your silver oxide compound. General Chemistry I (FC, 09 - 10) Lab #3: The Empirical Formula of a Compound Thus for the g of silver chloride in example 1: x % g silver chloride In this experiment, you will make two valid determinations of the empirical formula of an oxide of tin, which is a compound composed of only tin and oxygen.

You will take.

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Lab 1 determination of the empirical formula of silver oxide
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