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Alexandra [31]
3 years ago
14

A student performs a reaction that makes aluminum oxide. According to her calculations, she should expect to make 115.2 grams. S

he actually produces 66.9 grams. What is her percent yield?
Chemistry
1 answer:
tiny-mole [99]3 years ago
7 0

Answer:

The percentage of the student is 58.17%.

Explanation:

Expected yield of aluminum oxide = 115.2 g

Actual yield of aluminum oxide produced =66.9 g

The percentage yield is calculated by dividing actual yield by expected yield and then multiplying it with hundred.

Percentage yield:

\frac{\text{Actual yield}}{\text{Expected yield}}\times 100

\% Yield=\frac{66.9 g}{115.2 g}\times 100=58.17\%

The percentage of the student is 58.17%.

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If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K and then I raise the pressu
mixas84 [53]

Answer:

The answer to your question is V2 = 29.6 l

Explanation:

Data

Pressure 1 = P1 = 12 atm

Volume 1 = V1 = 23 l

Temperature 1 = T1 = 200 °K

Pressure 2 = 14 atm

Volume 2 = V2 = =

Temperature 2 = T2 = 300°K

Process

1.- To solve this problem use the Combine gas law.

             P1V1/T1 = P2V2/T2

-Solve for V2

             V2 = P1V1T2 / T1P2

2.- Substitution

             V2 = (12)(23)(300) / (200)(14)

3.- Simplification

             V2 = 82800 / 2800

4.- Result

            V2 = 29.6 l

5 0
3 years ago
Complete combustion of 8.10 g of a hydrocarbon produced 25.9 g of CO2 and 9.27 g of H2O. What is the empirical formula for the h
balu736 [363]

CxHy     +  O2    -->    x CO2     +    y/2  H2O

 

Find the moles of CO2 :     18.9g  /  44 g/mol   =    .430 mol CO2   = .430 mol of C in compound

Find the moles of H2O:      5.79g / 18 g/mol     =     .322 mol H2O   = .166 mol of H in compound

 

Find the mass of C and H in the compound:

                             .430mol  x 12  =  5.16 g C

                              .166mol  x 1g   = .166g H   

 

When you add these up they indicate a mass of 5.33 g for the compound, not 5.80g as you stated in the problem.

Therefore it is likely that either the mass of the CO2 or the mass of H20 produced is incorrect (most likely a typo).

In any event, to find the formula, you would take the moles of C and H and convert to a whole number ratio (this is usually done by dividing both of them by the smaller value).

8 0
4 years ago
You have a gas with a density of 4.8 grams per Liter and a molar mass of 75.3 grams per mole. How many liters of gas do you have
Andre45 [30]

d = √((x1 - x2)2 + (y1 - y2)2)  

( -2 , 5 )   ( 12 , -1 )    

  ↑    ↑         ↑     ↑      

 x1    y1        x2    y2  

d = √((-2 - 12)2 + (5 - (-1))2) = √((-14)2 + 62) = √(196 + 36) = √232 = 2√58 ≈ 15.23

7 0
3 years ago
Which statement is always true about a reversible chemical reaction?
Doss [256]

Answer: b

Explanation:

8 0
2 years ago
Crambury glasses made by adding?<br><br> Gold<br> Manganese<br> Cobalt <br> Chromium
Nataliya [291]

Answer:

Gold

Explanation:

Cranberry glass or 'Gold Ruby' glass is a red glass made by adding gold salts or colloidal gold to molten glass. Tin, in the form of stannous chloride, is sometimes added in tiny amounts as a reducing agent.

7 0
3 years ago
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