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4 years ago

Over-encouraging lesser skilled players can lead to embarrassment. a. True b. False

Chemistry

2 answers:

Alex Ar [27]4 years ago

7 0

Answer: Option (a) is correct.

Explanation:

A person with less skills needs to work more or practice more on his abilities in order to improve their athletic ability to build a stronger team.

Over encouragement to lesser skilled person can lead to the development of over confidence. As after over encouragement, the less skilled person can have the illusion of knowing each and everything which is not true for anyone.

As no one is perfect, therefore, over-encouraging lesser skilled players can lead to embarrassment.

Margarita [4]4 years ago

6 0

My answer would be a. True

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PLEASE HELP! 25 POINTS!!!! I got the #1, just not #2 and #3. An industrial chemical company has opened a new plant that will pro

podryga [215]

Answer :

Part 1 : Balanced reaction, $3H_2(g)+N_2(g)\rightarrow 2NH_3(g)$

Part 2 : The theoretical yield of $NH_3$ gas = 440.96 g

Part 3 : The % yield of ammonia is 90.03 %

Solution : Given,

Mass of $N_2$ = 475 g

Molar mass of $N_2$ = 28 g/mole

Molar mass of $NH_3$ = 17 g/mole

Experimental yield of $NH_3$ = 397 g

Answer for Part (1) :

The balanced chemical reaction is,

$3H_2(g)+N_2(g)\rightarrow 2NH_3(g)$

Answer for Part (2) :

First we have to calculate the moles of $N_2$ .

$\text{Moles of }N_2=\frac{\text{ Mass of }N_2}{\text{ Molecular mass of }N_2}=\frac{475g}{28g/mole}=16.96moles$

From the given reaction, we conclude that

1 moles of $N_2$ gas react to give 2 moles of $NH_3$ gas

16.96 moles of $N_2$ gas react to give $\frac{2}{1}\times 16.96=33.92$ moles of $NH_3$ gas

Now we have to calculate the mass of $NH_3$ gas.

$\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3$

$\text{ Mass of }NH_3=(33.92moles)\times (17g/mole)=440.96g$

Therefore, the theoretical yield of $NH_3$ gas = 440.96 g

Answer for Part (3) :

Formula used for percent yield :

$\% \text{ yield of }NH_3=\frac{\text{ Experimental yield of }NH_3}{\text{ Theoretical yield of }NH_3}\times 100$

$\% \text{ yield of }NH_3=\frac{397g}{440.96g}\times 100=90.03\%$

Therefore, the % yield of ammonia is 90.03 %

3 0

3 years ago

Neon doesn't take part in chemical reaction why give reason

ankoles [38]

Neon has filled its outer shells, therefore it is very stable and does not need to react with other elements and doesn’t form compounds.

5 0

3 years ago

Read 2 more answers

Calculate the mole fraction of benzene in a mixture that contains 45.2 g of benzene and 115.8 g of toluene.

ololo11 [35]

molecular weight of toluene = 92 g/mol

C6 = 12 x 6 = 72

H5 = 1 x 5 =5

CH3 = 12 + 1 x 3 =15

molecular weight of benzene = 78 g/mol

C6 = 12 x 6 = 72

H6 = 1 x 6 = 6

moles toluene:

115.8 / (92 g/mol) = 1.25 mol

moles benzene:

45.2/ (78 g/mol) = 0.57mol

total moles: 1.25 + 0.57= 1.82 moles

mole fraction of toluene:

1.25 mol / 1.82 moles = 0.68

6 0

4 years ago

What is the difference between bonds holding together atoms and forces between molecules?

Maksim231197 [3]

Written Answer: Covalent bonds hold atoms together in molecules and polyatomic ions where as intermolecular forces hold molecules together in a liquid or solid. Intermolecular forces are generally much weaker than covalent bonds.

Explanation/Evidence: "In contrast to intramolecular forces, such as the covalent bonds that hold atoms together in molecules and polyatomic ions, intermolecular forces hold molecules together in a liquid or solid. Intermolecular forces are generally much weaker than covalent bonds."

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3 years ago

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julsineya [31]

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10mg/kg and the tylenol is 80 mg per tables.
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3 years ago