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Basile [38]
2 years ago
11

CaCO3 → CaO + CO2 Calculate the theoretical yield of Calcium Oxide if 24.8 grams of Calcium Carbonate decomposes. Calculate the

percent yield if you got 13.1 grams in the laboratory.
Chemistry
1 answer:
RideAnS [48]2 years ago
5 0

Answer:

Theoretical yield: 13.9 g

Percent yield: 94 %

Explanation:

The reaction is:

CaCO₃ → CaO + CO₂

We see that the reaction is correctly balanced.

1 mol of calcium carbonate can decompose to 1 mol of calcium oxide and 1 mol of carbon dioxide.

We convert the mass to moles: 24.8 g . 1mol / 100.08g = 0.248 moles

As ratio is 1:1, 0.248 moles of salt can decompose to 1 mol of oxide.

We convert the moles to mass: 0.248 mol . 56.08g /1mol = 13.9 g

That's the theoretical yield.

To determine the percent yield we think:

(Determined yield / Theoretical yield) . 100 → (13.1 / 13.9) . 100 = 94 %

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wariber [46]

Answer:

Adding sodium or potassium hydroxide in amounts sufficient to convert all the H2SO4 into Na2SO4 would approximately neutralize the solution. The error would be the result of the imbalance between the basicity of the hydroxide and the acidity of the bisulfate (HSO4) anion. An adjustment in concentration would have to be made to achieve an accurate approximate pH of 7. But then you didn’t ask how much we would need to add.

Explanation:

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4 0
3 years ago
Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 3.56 mol of m
pishuonlain [190]
<h3>Answer:</h3>

43.27 g Mg

<h3>Explanation:</h3>

The balanced equation for the reaction between magnesium metal and hydrochloric acid is;

Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

From the equation;

1 mole of magnesium reacts with 2 moles of HCl

We are given;

3.56 moles of Mg and 3.56 moles of HCl

Using the mole ratio;

3.56 moles of Mg would react with 7.12 moles of HCl, and

3.56 moles of HCl would react with 1.78 moles of Mg

Therefore;

The amount of magnesium was in excess;

Moles of Mg left = 3.56 moles - 1.78 moles

                         = 1.78 moles

But; 1 mole of Mg = 24.305 g/mol

Therefore;

Mass of magnesium left = 1.78 moles × 24.305 g/mol

                                        = 43.2629 g

                                        = 43.27 g

Thus, the mass of magnesium that remained after the reaction is 43.27 g

4 0
3 years ago
A mixture of co(g) and h2(g) is pumped into a previously evacuated 2l reaction vessel the total pressure of the reaction system
swat32

Answer is: total pressure of the system is 2.4 atm.

Boyle's Law (the pressure volume law): volume of a given amount of gas held  varies inversely with the applied pressure when the temperature and mass are constant.

p₁V₁ = p₂V₂ (the product of the initial volume and pressure is equal to the product of the volume and pressure after a change).

1.2 atm · 2 L = p₂ · 1 L.

p₂ = 1.2 atm · 2 L / 1 L.

p₂ = 2.4 atm.

When pressure goes up, volume goes down.  

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7 0
3 years ago
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What will Number 17 be?
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The unbalanced Equation is
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4 0
3 years ago
You have 49.8 g of O2 gas in a container with twice the volume as one with CO2 gas. The pressure and temperature of both contain
IrinaVladis [17]

Answer:

34.2 g is the mass of carbon dioxide gas one have in the container.

Explanation:

Moles of O_2:-

Mass = 49.8 g

Molar mass of oxygen gas = 32 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{49.8\ g}{32\ g/mol}

Moles_{O_2}= 1.55625\ mol

Since pressure and volume are constant, we can use the Avogadro's law  as:-

\frac {V_1}{n_1}=\frac {V_2}{n_2}

Given ,  

V₂ is twice the volume of V₁

V₂ = 2V₁

n₁ = ?

n₂ = 1.55625 mol

Using above equation as:

\frac {V_1}{n_1}=\frac {V_2}{n_2}

\frac {V_1}{n_1}=\frac {2\times V_1}{1.55625}

n₁ = 0.778125 moles

Moles of carbon dioxide = 0.778125 moles

Molar mass of CO_2 = 44.0 g/mol

Mass of CO_2 = Moles × Molar mass = 0.778125 × 44.0 g = 34.2 g

<u>34.2 g is the mass of carbon dioxide gas one have in the container.</u>

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3 years ago
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