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Marizza181 [45]
3 years ago
9

A sample of CaCO3(s) is introduced into a sealed container of volume 0.638 L and heated to 1000 K until equilibrium is reached.

The Kp for the reaction CaCO3(s)⇌CaO(s)+CO2(g) is 3.8×10−2 at this temperature. Calculate the mass of CaO(s) that is present at equilibrium.
Chemistry
1 answer:
JulsSmile [24]3 years ago
7 0

Answer:

the mass of CaO present at equilibrium is, 0.01652g

Explanation:

K_p = [CO_2] = 3.8×10⁻²

Now we have to calculate the moles of CO₂

Using ideal gas equation,

PV =nRT

P = pressure of gas = 3.8×10⁻²

T = temperature of gas = 1000 K

V = volume of gas = 0.638 L

n = number of moles of gas = ?

R = gas constant = 0.0821 L.atm/mole.k

\frac{3.8 * 10^2 * 0.638}{0.0821 * 1000} \\= 2.95 * 10^-^4

Now we have to calculate the mass of CaO

mass = 2.95 * 10 ⁻⁴ × 56

= 0.01652g

Therefore,

the mass of CaO present at equilibrium is, 0.01652g

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Explanation:

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1. Calculate the RFM of Fe(NO3)2
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Explanation:

The Relative Formula Mass is the mass of one mole of a compound expressed in grams, obtained by adding together the Relative Atomic Masses, RAM, of the elements which makes the compound

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The relative formula mass of Fe(NO₃)₂ is given as follows;

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The relative atomic mass of oxygen, O = 15.999 amu

Therefore, we have;

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5 0
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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
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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

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Where, H = Heat absorbed

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c = specific heat capacity of the metal

dT = temperature change

Putting the values in the equation

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c = 385 JKg-1°C-1

Thus, the metal is copper.

Learn more about specific heat

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