1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
AysviL [449]
2 years ago
11

Twenty five grams of Iron 3 oxide react with an excess of carbon monoxide to form 15 g of Fe. Carbon dioxide is the other produc

t. Calculate the theoretical yield and the percent yield of iron.
Chemistry
1 answer:
densk [106]2 years ago
7 0
<h3>Answer:</h3>

Theoretical mass = 17.42 g

Percent yield of Fe = 86.11%

<h3>Explanation:</h3>

The equation for the reaction between iron (iii) oxide and carbon monoxide is given by;

Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)

We are required to calculate the theoretical yield and the percentage yield of Iron.

Step 1: Moles of iron (iii) oxide

Moles are given by dividing the mass of the compound by the molar mass.

Molar mass of Iron(iii) oxide = 159.69 g/mol

Moles of Iron(III) oxide = 25 g ÷ 159.69 g/mol

                                     = 0.156 moles

Step 2: Moles of Iron produced

From the equation 1 mole of Iron(iii) oxide reacts to produce 2 moles of Fe.

Therefore, the mole ratio of Fe₂O₃ to Fe is 1 : 2.

Thus, moles of Fe = Moles of Fe₂O₃ × 2

                              = 0.156 moles × 2

                              = 0.312 moles

Step 3: Theoretical mass of iron produced

To calculate the mass of iron we multiply the number of moles of iron with the relative atomic mass.

Relative atomic mass = 55.845

Mass of iron = 0.312 moles × 55.845

                    = 17.42 g

Step 4: Percent yield of iron

% yield = (Actual mass ÷ Theoretical mass)×100

            = (15 g ÷ 17.42 g) × 100 %

            = 86.11%

You might be interested in
Calcium Carbonate reacts with dilute hydrochloric acid. The equation for the reaction is shown. CaCo3 + 2Hcl = Cacl2 + H2O + Co2
Elena-2011 [213]

Answer:

Approximately 0.224\;\rm L, assuming that this reaction took place under standard temperature and pressure, and that \rm CO_2 behaves like an ideal gas. Also assume that the reaction went to completion.

Explanation:

The first step is to find out: which species is the limiting reactant?

Assume that \rm CaCO_3 is the limiting reactant. How many moles of \rm CO_2 would be produced?

Look up the relative atomic mass of \rm Ca, \rm C, and \rm O on a modern periodic table:

  • \rm Ca: 40.078.
  • \rm C: 12.011.
  • \rm O: 15.999.

Calculate the formula mass of \rm CaCO_3:

\begin{aligned} & M(\rm CaCO_3) \\ &= 40.078 + 12.011 + 3 \times 15.999 \\&= 100.086\; \rm g \cdot mol^{-1}\end{aligned}.

Calculate the number of moles of formula units in 1\; \rm g of \rm CaCO_3 using its formula mass:

\begin{aligned}& n(\mathrm{CaCO_3})\\&= \frac{m(\mathrm{CaCO_3})}{M(\mathrm{CaCO_3})} \\ &= \frac{1\; \rm g}{100.086\; \rm g \cdot mol^{-1}} \approx 1.00\times 10^{-2}\; \rm mol\end{aligned}.

In the balanced chemical equation, the ratio between the coefficient of \rm CaCO_3 and that of \rm CO_2 is \displaystyle \frac{n(\mathrm{CO_2})}{n(\mathrm{CaCO_3})} = 1.

In other words, for each mole of \rm CaCO_3 formula units consumed, one mole of \rm CO_2 would be produced.

If \rm CaCO_3 is indeed the limiting reactant, all that approximately 1.00\times 10^{-2}\; \rm mol of \rm CaCO_3\! formula would be consumed. That would produce approximately 1.00\times 10^{-2}\; \rm mol\! of \rm CO_2.

On the other hand, assume that \rm HCl is the limiting reactant.

Convert the volume of \rm HCl to \rm dm^{3} (so as to match the unit of concentration.)

\begin{aligned}&V(\mathrm{HCl})\\ &= 50\; \rm cm^{3} \\ &= 50\; \rm cm^{3} \times \frac{1\; \rm dm^{3}}{10^{3}\; \rm cm^{3}} \\ &= 5.00\times 10^{-2}\; \rm dm^{3} \end{aligned}.

Calculate the number of moles of \rm HCl molecules in that 5.00\times 10^{-2}\; \rm dm^{3} of this \rm 0.05\; \rm mol \cdot dm^{-3}

\begin{aligned}& n(\mathrm{HCl}) \\ &= c(\mathrm{HCl}) \cdot V(\mathrm{HCl}) \\ &= 0.05\; \rm mol \cdot dm^{-3}\\ &\quad\quad \times 5.00\times 10^{-2}\;\rm dm^{3} \\ &= 2.50 \times 10^{-3}\; \rm mol\end{aligned}.

Notice that in the balanced chemical reaction, the ratio between the coefficient of \rm HCl and that of \rm CO_2 is \displaystyle \frac{n(\mathrm{CO_2})}{n(\mathrm{HCl})} = \frac{1}{2}.

In other words, each mole of \rm HCl molecules consumed would produce only 0.5\;\rm mol of \rm CO_2 molecules.

Therefore, if \rm HCl is the limiting reactant, that 2.50 \times 10^{-3}\; \rm mol of \rm HCl\! molecules would produce only one-half as many (that is, 1.25\times 10^{-3}\; \rm mol) of \rm CO_2 molecules.

If \rm CaCO_3 is the limiting reactant, \rm 1.00\times 10^{-3}\; \rm mol of \rm CO_2 molecules would be produced. However, if \rm HCl is the limiting reactant, 1.25\times 10^{-3}\; \rm mol of \rm CO_2\! molecules would be produced.

In reality, no more than \rm 1.00\times 10^{-3}\; \rm mol of \rm CO_2 molecules would be produced. The reason is that all \rm CaCO_3 would have been consumed before \rm HCl was.

After finding the limiting reactant, approximate the volume of the \rm CO_2\! produced.

Assume that this reaction took place under standard temperature and pressure (STP.) Under STP, the volume of one mole of ideal gas molecules would be approximately 22.4\; \rm L.

If \rm CO_2 behaves like an ideal gas, the volume of that \rm 1.00\times 10^{-3}\; \rm mol of \rm CO_2\! molecules would be approximately \rm 1.00\times 10^{-3}\; \rm mol \times 22.4\; \rm L = 0.224\; \rm L.

3 0
3 years ago
What is the equilibrium constant for the reaction<br> SO2(g) + NO2(g) = S03(g) + NO(g)?
aev [14]

Answer:

Keq: [SO3][NO] /[SO2]NO2]

Explanation:

3 0
1 year ago
Can anyone help me with my chemistry question?
loris [4]
Hi!


1) electrons
2) Chadwick
3) J. J. Thompson
4) Bohr
5) Rutherford
6) Dalton
7) Nucleus


I hope this helps!
5 0
3 years ago
During diffusion which way do the substances move?
ser-zykov [4K]
During diffusion substances move from the denser medium (meaning where there is more of the substance) to less dense medium (meaning where there is less of the substance).


3 0
3 years ago
Identify the units used to measure volume mass.
Strike441 [17]

Answer:

The metric system uses units such as meter, liter, and gram to measure length, liquid volume, and mass, just as the U.S. customary system uses feet, quarts, and ounces to measure these.

Volume: 1 liter is a little more than 1 quart

Mass: 1 kilogram is a little more than 2 pounds

Length: 1 centimeter is a little less than half an

Explanation:

3 0
2 years ago
Other questions:
  • Hydrogen gas and gaseous iodine will react to form hydrogen iodide, as described by the following chemical equation.H2(g)+I2(g)↽
    15·1 answer
  • A 7.85 × 10-5 mol sample of copper-61 emits 1.47 × 1019 positrons in 90.0 minutes. what is the decay constant for copper-61
    12·1 answer
  • A chemical reaction gives off 2100 kg of heat energy how many calories
    7·1 answer
  • Which of the following statements is true about cellular respiration?
    6·2 answers
  • For an object that is speeding up at a constant rate, how would the acceleration vs. time graph look?
    14·2 answers
  • How many moles of sodium bicarbonate is needed to neutralize 0.8 ml of sulphuric acid?
    8·1 answer
  • What energy is required for a reaction to occur?
    11·2 answers
  • The block in this illustration is floating in water, which has a density of 1.00 g/cm3 .What is a good estimate of the density o
    11·1 answer
  • El champú ¿es de naturaleza básica o acida? ¿Como puedes saberlo?
    11·1 answer
  • A 2. 26 l balloon of helium is at 30°c and 1. 61 atm, what is the pressure if the volume is increased to 4. 12 l?.
    9·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!