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Cerrena [4.2K]
3 years ago
8

how do you tell if an element has positive or negative charge. And how do you know when the valence electrons have to be shared

or not​
Chemistry
1 answer:
Eva8 [605]3 years ago
7 0

Answer:

A normal atom has a neutral charge. When you are missing electrons it has a positive charge. When you have extra electron, you have a negative charge. I am not sure what the answer to your second question is, sorry.

Explanation:

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What part of the microscope is the letter k?
snow_tiger [21]

Answer:

if you are asking k then the round one is condenser

if not then its a stage clip

6 0
3 years ago
How do you test for carbon dioxide ?? Explain
g100num [7]

Answer:

Carbon dioxide reacts with calcium hydroxide solution to produce a white precipitate of calcium carbonate

Explanation:

. Limewater is a solution of calcium hydroxide. If carbon dioxide is bubbled through limewater, the limewater turns milky or cloudy white

5 0
2 years ago
Ethyl butyrate, CH3CH2CH2CO2CH2CH3, is an artificial fruit flavor commonly used in the food industry for such flavors as orange
SIZIF [17.4K]

Answer:

A. 10.0 grams of ethyl butyrate would be synthesized.

B. 57.5% was the percent yield.

C. 7.80 grams of ethyl butyrate would be produced from 7.60 g of butanoic acid.

Explanation:

CH_3CH_2CH_2CO_2H(l)+CH_2CH_3OH(l)+H^+\rightarrow CH_3CH_2CH_2CO_2CH_2CH_3(l)+H_2O(l)

A

Moles of butanoic acid = \frac{7.60 g}{88 g/mol}=0.08636 mol

According to reaction ,1 mole of butanoic acid gives 1 mol of ethyl butyrate,then 0.08636 mol of butanoic acid will give :

\frac{1}{1}\times 0.08636 mol=0.08636 mol of ethyl butyrate

Mass of 0.08636 moles of ethyl butyrate =

0.08636 mol × 116 g/mol = 10.0 g

Theoretical yield = 10.0 g

Experimental yield = ?

Percentage yield of the reaction = 100%

Yield\%=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

100\%=\frac{\text{Experimental yield}}{10.0 g}\times 100

Experimental yield = 10.0 g

10.0 grams of ethyl butyrate would be synthesized.

B

Theoretical yield of ethyl butyrate  = 10.0 g

Experimental yield ethyl butyrate = 5.75 g

Percentage yield of the reaction = ?

Yield\%=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

=\frac{5.75 g}{10.0 g}\times 100=57.5\%

57.5% was the percent yield.

C

Moles of butanoic acid = \frac{7.60 g}{88 g/mol}=0.08636 mol

According to reaction ,1 mole of butanoic acid gives 1 mol of ethyl butyrate,then 0.08636 mol of butanoic acid will give :

\frac{1}{1}\times 0.08636 mol=0.08636 mol of ethyl butyrate

Mass of 0.08636 moles of ethyl butyrate =

0.08636 mol × 116 g/mol = 10.0 g

Theoretical yield = 10.0 g

Experimental yield = ?

Percentage yield of the reaction = 78.0%

Yield\%=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

78.0\%=\frac{\text{Experimental yield}}{10.0 g}\times 100

Experimental yield = 7.80 g

7.80 grams of ethyl butyrate would be produced from 7.60 g of butanoic acid.

8 0
3 years ago
4. At what temperature will 1.21 mol of oxygen (O2), exert a pressure of 1862 mmHg in a
Airida [17]

Answer:

Pressure = 1820 mmHg ... T = ( 2.39atm x 5.12L ) / ( 0.4041 moles x 0.08206atm. ... n is moles, R is the gas constant, and T is temperature in Kelvins.

Explanation:

this might help you

7 0
2 years ago
What is the difference between the equilibrium position and the equilibrium constant of a reaction? Which changes as a result of
maria [59]

If the concentrations of the substances present in the equilibrium are adjusted, the equilibrium constants remain unchanged. An equilibrium constant can only be altered by a change in temperature. If you adjust the concentration of something present in the mixture, the equilibrium position will change.

Equilibrium Constant vs. Equilibrium Position: The Difference

Equilibrium position is the point at which the forward reaction of the equilibrium is equal to the backward reaction, whereas equilibrium constant is the number that describes the connection between amounts of products and reactants of a reaction mixture at its equilibrium. The main distinction between equilibrium position and equilibrium constant is this.

To know more about Equilibrium Constant vs. Equilibrium Position

brainly.com/question/24175270

#SPJ4

3 0
2 years ago
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