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spayn [35]
3 years ago
5

2Fe2O3+3C_4Fe+3 CO2 how many moles of Carbon are needed to produce 1.9 moles of iron (Fe)?​

Chemistry
1 answer:
Bad White [126]3 years ago
7 0
Um use English no offense
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What is the percentage error of length measurement of 0.229cm if the correct value is 0.225cm
Mars2501 [29]

Percent error is the difference between the measured and known value, divided by the known value, multiplied by 100%.

So first, we take our measured value, .299 cm, minus our known value, .225 cm.

.299 cm - .225 cm=.004 cm

Next, we divide that by our known value

\frac{.004}{.225}=.0177777778

Finally, multiply your answer by 100

.0177777778 x 100= 1.77777778 %

Round to three significant figures, and you're done.

=1.78 % error



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Why do foods and fuels have chemical potential energy?
Ainat [17]
Fuels are burned to produce energy, and your body breaks down the food to produce nutrients for your body.
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A sample of metal has a mass of 5. 2 g and absorbs 20. 0 j of energy as it is heated from 30. 0°c to 40. 0°c. What is the identi
kiruha [24]

The identity of the metal is copper.

<h3>What is specific heat?</h3>

The amount of energy needed to raise the temperature of one gram of a substance by one degree Celsius.

Using the formula of specific heat

H = mcdT

Where, H = Heat absorbed

m = mass of the metal

c = specific heat capacity of the metal

dT = temperature change

Putting the values in the equation

20 J = 0.0052 Kg × c × ( 40.0°C - 30.0°C)

c = 20 J/0.0052 Kg × ( 40.0°C - 30.0°C)

c = 385 JKg-1°C-1

Thus, the metal is copper.

Learn more about specific heat

brainly.com/question/11297584

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2 years ago
All the members of this family (inner transition metals) are both ______________ and _____________.
avanturin [10]

Answer:

The actinides and the lanthanides

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3 years ago
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Determine the mole fractions and partial pressures of CO2, CH4, and He in a sample of gas that contains 1.20 moles of CO2, 1.79
BARSIC [14]

Answer :  The mole fraction and partial pressure of CH_4,CO_2 and He gases are, 0.267, 0.179, 0.554 and 1.54, 1.03 and 3.20 atm respectively.

Explanation : Given,

Moles of CH_4 = 1.79 mole

Moles of CO_2 = 1.20 mole

Moles of He = 3.71 mole

Now we have to calculate the mole fraction of CH_4,CO_2 and He gases.

\text{Mole fraction of }CH_4=\frac{\text{Moles of }CH_4}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}

\text{Mole fraction of }CH_4=\frac{1.79}{1.79+1.20+3.71}=0.267

and,

\text{Mole fraction of }CO_2=\frac{\text{Moles of }CO_2}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}

\text{Mole fraction of }CO_2=\frac{1.20}{1.79+1.20+3.71}=0.179

and,

\text{Mole fraction of }He=\frac{\text{Moles of }He}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}

\text{Mole fraction of }He=\frac{3.71}{1.79+1.20+3.71}=0.554

Thus, the mole fraction of CH_4,CO_2 and He gases are, 0.267, 0.179 and 0.554 respectively.

Now we have to calculate the partial pressure of CH_4,CO_2 and He gases.

According to the Raoult's law,

p_i=X_i\times p_T

where,

p_i = partial pressure of gas

p_T = total pressure of gas  = 5.78 atm

X_i = mole fraction of gas

p_{CH_4}=X_{CH_4}\times p_T

p_{CH_4}=0.267\times 5.78atm=1.54atm

and,

p_{CO_2}=X_{CO_2}\times p_T

p_{CO_2}=0.179\times 5.78atm=1.03atm

and,

p_{He}=X_{He}\times p_T

p_{He}=0.554\times 5.78atm=3.20atm

Thus, the partial pressure of CH_4,CO_2 and He gases are, 1.54, 1.03 and 3.20 atm respectively.

4 0
3 years ago
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