CHEMISTRY COLLEGE

1. Based on the appearance of your reaction in the beaker, which reagent do you think was consumed and which reagent had some left over? The aluminum was consumed, and copper was left over as seen by the reddish particles. 2. If 5.0 g of iron metal is reacted with 15.0 g of Cl2 gas, how many grams of ferric chloride will form? About 14.52 grams will form. 3. For the reaction above the amount of ferric chloride obtained in the lab was 9.15 grams. Calculate the percent yield. The percent yield would be around 63.02%. 4. What are some reasons for obtaining a percent yield of less than 100 percent? Factors such as the reactants not reacting completely, human error in the experiment, the reactants might have too large of a surface area for reaction, multiple reactions occurring within an experiment, temperature, etc.

Answers

Answer 1

Answer:

Answer:

1. Al is consumed first and CuSO₄ remains left.

2. The grams of ferric chloride that forms is 14.5 g.

3. The percent yield is 63.1%

4. Trace of impurities present in the reagents, bad manipulations when preparing solutions, etc.

Explanation:

1. The reaction is:

2Al + 3CuSO₄ = Al₂(SO₄)₃ + 3Cu

The number of moles of Al is less than the number of moles of CuSO₄. Therefore, Al is the limiting reagent and CuSO₄ is the excess reagent. This means that Al is consumed first and CuSO₄ remains left.

2. The reaction is:

2Fe + 3Cl₂ = 2FeCl₃

The number of moles of Fe is:

$n_(Fe) =(m_(Fe) )/(MW_(Fe) ) =(5)/(55.85) =0.0895moles$

The number of moles of Cl₂ is:

$n_(Cl2) =(15)/(70.9) =0.211moles$

We know that 2 moles of Fe react with 3 moles of Cl₂, thus:

2 moles Fe---------------3 moles Cl₂

0.0895 moles Fe-------X moles Cl₂

Clearing X:

$Xmoles_(Cl2) =(3*0.0895)/(2) =0.134moles$

It needs 0.134 moles of Cl₂ but it only has 0.211 moles, thus, Cl₂ is the excess reagent. Fe is the limiting reagent.

2 moles Fe-----------2 moles FeCl₃

0.0895 moles Fe------X moles FeCl₃

Clearing X:

$Xmoles_(FeCl3) =(2*0.0895)/(2) =0.0895moles$

$m_(FeCl3) =0.0895molesFeCl3*(162.2gFeCl3)/(1molFeCl3) =14.5g$

3. The actual yield of FeCl₃ is 9.15 g, the theoritical yield is 14.5 g, thus, ther percent yield is:

$Percent-yield=(Actual-yield)/(Theoritical-yield) *100=(9.15)/(14.5) *100=63.1$ %

4. Trace of impurities present in the reagents, bad manipulations when preparing solutions, etc.

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What would cause the percent yield of a reaction to be less than 100%?All of the limiting reagent gets used up.

The product participates in a side reaction.

Pure reactants are used.

A balanced chemical equation is used.

Answers

The product participates in a side reaction.

Explanation:

The reason why percentage yield for a chemical reaction can be less than a 100% is due to the presence of competing side reactions. As often the case and basics for all chemical reactions, mass and matter must be conserved. But sometimes the yield can be lower due to other reactions that must be considered.

A competing side reaction that can affect the yield of products during a chemical procedure is often one in which some of the products can react with some molecules present in the environment or some of the unused reactants when available.
Sometimes, a product can be hygroscopic, deliquescent or probably effervescent. This will definitely alter the expected amount of product one desires in a reaction based on stoichiometry.

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Answer:

The product participates in a side reaction.

Explanation:

Write the balanced reaction and solubility product expression (KSP) for dissolving silver chromate: Ag2CrO4(s). Include all charges, stoichiometric coefficients, and phase subscripts.

Answers

Answer:

2Ag⁺ (aq) + CrO₄⁻² (aq) ⇄ Ag₂CrO₄ (s) ↓

Ksp = [2s]² . [s] → 4s³

Explanation:

Ag₂CrO₄ → 2Ag⁺ + CrO₄⁻²

Chromate silver is a ionic salt that can be dissociated. When we have a mixture of both ions, we can produce the salt which is a precipitated.

2Ag⁺ (aq) + CrO₄⁻² (aq) ⇄ Ag₂CrO₄ (s) ↓ Ksp

That's the expression for the precipitation equilibrium.

To determine the solubility product expression, we work with the Ksp

Ag₂CrO₄ (s) ⇄ 2Ag⁺ (aq) + CrO₄⁻² (aq) Ksp

2 s s

Look the stoichiometry is 1:2, between the salt and the silver.

Ksp = [2s]² . [s] → 4s³

A car is traveling at 87.0 km/hr. How many meters will it travel in 37.0 seconds?

Answers

Speed of the car = $87.0 (km)/(hr)$

Given time = 37.0 s

Converting time from seconds to hours:

1 hr= 60 min; 1 min = 60 s

$37.0 s * (1 min)/(60s)*(1 hr)/(60min) = 0.0103 hr$

Calculating distance from speed and time:

$0.0103 hr * (87.0 km)/(1 hr) =0.894 km$

Converting distance from km to m:

$0.894 km * (1000 m)/(1 km) = 894 m$

So the distance traveled by the car in 37.0 s is 894 m.

Which of the following do you need to know to be able to calculate the molarity of a salt solution ? I. the mass of salt added II. the molar mass of the salt III. the volume of water added IV. the total volume of the solution A) II and III only B) I, II, and IV only C) I, II, and III only D) I and III only E) You need all of the information.

Answers

According to molar concentration, for calculating molarity of salt solution mass,molar mass of salt and volume of solution is required , hence option B is correct.

What is molar concentration?

Molar concentration is defined as a measure by which concentration of chemical substances present in a solution are determined. It is defined in particular reference to solute concentration in a solution . Most commonly used unit for molar concentration is moles/liter.

The molar concentration depends on change in volume of the solution which is mainly due to thermal expansion. Molar concentration is calculated by the formula, molar concentration=mass/ molar mass ×1/volume of solution in liters.

In terms of moles, it's formula is given as molar concentration= number of moles /volume of solution in liters.

Learn more about molar concentration,here:

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Explanation:

to find molarity

1the mass of salt added

Find the number of moles of solute dissolved in solution,

2 molar mass of salt

Find the volume of solution in liters,

4 total volume of solution

so B

Joan has four containers. The chart below shows the mass and volume of each of the containers. Two of the containers are filled with solids, one is filled with a liquid, and one is filled with a gas.

Answers

Answer:

This question is incomplete

Explanation:

This question is incomplete. However, it should be noted that if the containers are compared with an equal average volume, the containers having solids will have larger masses than that containing liquid which will also have a larger mass than that containing gas. This is because solids have there molecules touching each other in compact manner which makes the molecule exert a certain combined force/mass. The molecules of liquid are also close to one another but are not compact like the solids and are hence exerting a lesser force/mass than solids. Gases have free molecules that are far apart and thus are usually the lightest when they occupy the same volume as liquids and solids.

A gas mixture with a total pressure of 770 mmHg contains each of the following gases at the indicated partial pressures: 128 mmHg CO2, 232 mmHg Ar, and 183 mmHg O2. The mixture also contains helium gas. What is the partial pressure of the helium gas?

Answers

The partial pressure of Helium gas can be calculated by applying Daltons law of partial pressure and that comes out to be 227 mmHg.

What is Dalton's law of partial pressure?

Dalton's law of partial pressure helps in calculating the total pressure exerted by all the gases that are present in a mixture that is equal to the sum of partial pressure of all individual gases.

Partial pressure is the pressure that is exerted by one gas in a mixture of gases on the walls of the container. This law is applicable to only mixture of gases that are ideal gases. Ideal gases are the one which do not have any forces of attraction or repulsion between the particles of thee gas.

In our question

$p_(total) =p_{CO_(2) }+p_(Ar)+p_{O_(2) } +p_{{He} }$