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nadya68 [22]
3 years ago
15

When 2.3 × 10^3 g of CaCO3 are heated, the actual yield of CaO is 1.09 × 10^3g. What is

Chemistry
1 answer:
iren [92.7K]3 years ago
5 0

The percent yield : 4. 84.58%

<h3>Further explanation</h3>

Reaction

CaCO₃ ⇄ CaO+CO₂

mass CaCO₃ = 2.3 × 10³ g

mol CaCO₃ (MW=100.0869 g/mol) :

\tt mol=\dfrac{mass}{MW}\\\\mol=\dfrac{2.3\times 10^3}{100,0869}\\\\mol=22.98

From the equation, mol CaCO₃ : CaO = 1 : 1, so mol CaO=22.98

mass CaO(MW=56.0774 g/mol)⇒ (theoretical) :

\tt mass=mol\times MW\\\\mass=22.98\times 56,0774\\\\mass=1288.659~g

The percent yield :

\tt \%yield=\dfrac{actual}{theoretical}\times 100\%\\\\\%yield=\dfrac{1090}{1288.659}\times 100\%\\\\\5yield=84.58\%

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According to collision and transition state theories, what is the importance of activation energy?
In-s [12.5K]

According to the collision theory, the following criteria must be met in order for a chemical reaction to occur: Molecules must collide with sufficient energy, known as the activation energy, so that chemical bonds can break.

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3 0
2 years ago
URGENT If you take four gas samples with the following pressures: 12.3 atm, 56.7 atm, 1.09 atm, and 32.6 atm. What is the total
Fittoniya [83]

The total pressure of gas samples are 102.69 atmosphere, if the gas samples have pressure of 12.3 atmosphere, 56.7 atmosphere, 1.09 atmosphere, and 32.6 atmosphere.

Explanation:

The given is,

                 Gas samples pressure are,

                 12.3 atmosphere, 56.7 atmosphere, 1.09 atmosphere, and 32.6 atmosphere

Step:1

              From the  Dalton’s Law of Partial Pressure,

              The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas,

                                    P_{Total} = P_{1} + P_{2} +P_{3} + P_{4}.........................(1)

              Where, P_{1} ,P_{2} ,P_{3}., etc. are the pressure of gas sample respectively 1,2,3.,etc.

Step:2

               From the given,

                                  P_{1} = 12.3 atmosphere    

                                  P_{2} = 56.7 atmosphere

                                  P_{3} = 1.09 atmosphere

                                  P_{4} = 32.6 atmosphere

                Equation (1) becomes,

                                       = 12.3 + 56.7 + 1.09 + 32.6

                                       = 102.69 atmosphere

                Total pressure of gas samples are = 102.69 atmosphere

Result:

              The total pressure of gas samples are 102.69 atmosphere, if gas samples have pressure of 12.3 atmosphere, 56.7 atmosphere, 1.09 atmosphere, and 32.6 atmosphere.

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<em>d =  \frac{m}{v}</em>

<em>d =  \frac{25.8}{10.3}</em>

<em>d =  2.5</em>

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