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AysviL [449]
3 years ago
12

How many liters of CO2 are formed when 14.0 g of CaCO3 react at 1.00 atm and 1000K

Chemistry
2 answers:
Gnesinka [82]3 years ago
7 0

Answer: 11.5

Explanation:

spin [16.1K]3 years ago
3 0

Answer : The volume of CO_2 formed are 11.5 liters.

Explanation :

First we have to calculate the moles of CaCO_3

\text{Moles of }CaCO_3=\frac{\text{Mass of }CaCO_3}{\text{Molar mass of }CaCO_3}

Molar mass of CaCO_3 = 100 g/mole

\text{Moles of }CaCO_3=\frac{14.0g}{100g/mole}=0.14mole

The balanced chemical reaction will be:

CaCO_3\rightarrow CaO+CO_2

From the balanced chemical reaction we conclude that,

As, 1 mole of CaCO_3 react to give 1 mole pf CO_2

So, 0.14 mole of CaCO_3 react to give 0.14 mole pf CO_2

Thus, the moles of CO_2 gas = 0.14 mole

Now we have to calculate the volume of CO_2.

Using ideal gas equation:

PV=nRT

where,

P = pressure of gas = 1.00 atm

V = volume of gas = ?

T = temperature of gas = 1000 K

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

n = moles of gas = 0.14 mole

Now put all the given values in the ideal gas equation, we get:

(1.00atm)\times V=(0.14mole)\times (0.0821L.atm/mole.K)\times (1000K)

V=11.5L

Therefore, the volume of CO_2 formed are 11.5 liters.

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