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3 years ago

A coin floats on the top of a glass of water. Explain why the coin is able to float on top of the water in this glass.

Chemistry

2 answers:

liberstina [14]3 years ago

6 0

The surface tension of the water.

Goshia [24]3 years ago

4 0

Answer:

The surface tension of the water

Explanation:

The surface of the water curves down twords the edge of the coin.

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Sliva [168]

2 HClO(aq) + Ca(OH)2(aq) = 2 H2O(l) + Ca(ClO)2(aq) is the balanced equation

4 0

3 years ago

If 4.50 g of HCl are reacted with 15.00 g of Caco, according to the following balanced chemical equation, calculate the theoreti

Tom [10]

Answer: HCl is the limiting reactant and the theoretical yield is 2.72 g of CO2. If the actual yield was 2.50 g then, the percent yield is 92.0% when rounding off is done only for the final answer.

Further Explanation:

In order to determine the theoretical yield and the percent yield of CO2, the following steps must be done:

Determine the limiting reactant. This is the reactant that will determine the amount of CO2 that will actually form.
Determine the theoretical yield for CO2 when the limiting reactant is used.
Get the percent yield by getting the ratio of the actual yield stated in the problem and the calculated theoretical yield multiplied by 100.

Determining the Limiting Reactant

The Limiting Reactant (LR) will produce fewer moles of the products. To check which of the reactants HCl or CaCO3 is the LR, we do dimensional analysis:

For HCl:

$moles\ CO_{2}\ = (4.50\ g\ HCl)\(\frac{1\ mol\ HCl}{36.46094\ g})( \frac{1\ mol\ CO_{2} }{2\ mol\ HCl}) \\moles\ CO_{2}\ =\ 0.0617098$

For CaCO3:

$moles\ of\ CO_{2}\ = (15.00\ g\ CaCO_{3})\ (\frac{1\ mol\ CaCO_{3} }{100.0869\ g\ CaCO_{3} })\ (\frac{1\ mol\ CO_{2} }{1\ mol\ CaCO_{3} })\\moles\ of\ CO_{2}\ = \ 0.1499$

Since HCl produces fewer moles of CO2, then it is the limiting reactant. We will use the given amount to determine the theoretical yield for CO2.

Determining the Theoretical Yield

From Step 1, we know that 0.0617098 moles of CO2 will be produced. We will just convert this to grams.

$grams\ CO_{2}\ =\ (0.0617098\ mol\ CO_{2}) (\frac{44.01\ g\ CO_{2}}{1\ mol\ CO_{2}})\\grams\ CO_{2}\ =\ 2.71585$

Since the answer only requires 3 significant figures, the final answer is 2.72 grams CO2.

Determining the Percent Yield

Dividing the actual yield by the theoretical yield will give us the percent yield, which is an indicator of how efficient the experiment or the method used was.

From the problem, the actual yield was 2.50 g, hence, the percent yield is:

$percent\ yield\ of\ CO_{2}\ = (\frac{2.50\ g}{2.71585\ g}) (100)\\percent\ yield\ of\ CO_{2}\ = 92.05221$

Rounding off to three significant figures, the percent yield is 92.0%. This suggests that the method used is somewhat efficient in producing CO2.

Learn More

Learn More about Limiting Reactant brainly.com/question/7144022
Learn More about Excess Reactant brainly.com/question/6091457
Learn More about Stoichiometry brainly.com/question/9743981

Keywords: stoichiometry, theoretical yield, actual yield

3 0

3 years ago

Carbon disulfide is produced by the reaction of carbon and sulfur dioxide. What is the percent yield of carbon disulfide if the

Akimi4 [234]

Answer:

The percent yield of carbon disulfide is 78.8%

Explanation:

Percent yield of reaction = (Produced yield / Theoretical yield) . 100

5C + 2SO₂ --> CS₂ + 4CO

In the reaction 5 moles of C, produce 1 mol of CS₂

40 g / 12 g/m = 3.33 moles

Then, this is the rule of three:

5 mol of C produce 1 mol of CS₂

3.33 moles of C, will produce ( 3.33 .1)/5 = 0.666 moles

Mol . molar mass = mass → 0.666 mol . 76.12 g/m =50.7 g (Theoretical yield)

(40 g / 50.7 g) . 100 = 78.8%

7 0

3 years ago

4Fe + 3O2 = 2Fe2O3: How many grams of Fe2O3 will be produced from 10 g of Fe and 7 g of O2?

bixtya [17]

If you know how to convert grams to moles, do that first. Then, use a b delta a table to find x. Then add 2x to 2Fe2O3 to get .08953 moles. Not shown in pic, that amount in grams is 14.2967

6 0

3 years ago

A sample of hydrogen is collected in a flask over water. The partial pressures are 736 torr for H2 and 22 torr for H2O. What tot

Dmitrij [34]

The total pressure exerted by the mixture of gases is 758 Torr.

Explanation:

Dalton's law of partial pressure is used to determine the total pressure exerted by mixture of gases. Also if we know the total pressure and the partial pressure of N-1 gases for mixture of N gases, then we can determine the partial pressure for the Nth gas.

So as per that law, the total pressure of any mixture of gases is equal to the sum of the partial pressure of individual gases. As partial pressure is the measure or the ability of each gas to produce pressure in a given volume, so the sum of those partial pressure will give the total pressure present in the gas mixture.

$Total pressure = Partial pressure of Hydrogen + Partial pressure of water.$

As the partial pressure of H₂ gas is given as 736 Torr and the partial pressure of H₂O is given as 22 Torr, the total pressure will be equal to the sum of those two pressures.

Total pressure = 736 + 22 = 758 Torr.

So, the total pressure exerted by the mixture of gases is 758 Torr.

8 0

3 years ago