CaCO3(s)⇄CaO(s)+CO2(g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxid
1 answer:
Answer:
1.04 mol
Explanation:
CO₂ is produced in a closed 100 L vessel according to the following equation.
CaCO₃(s) ⇄ CaO(s) + CO₂(g)
At equilibrium, the pressure of carbon dioxide remains constant at 1.00 atm.
First, we need to conver the temperature to the absolute scale (Kelvin scale) using the following expression.
K = °C + 273.15
K = 898°C + 273.15
K = 1171 K
Now, we can find the moles of carbon dioxide using the ideal gas equation.
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<h2>Hello!</h2>
The answer is:
The percent yield of the reaction is 32.45%
<h2>Why?</h2>To calculate the percent yield, we have to consider the theoretical yield and the actual yield. The theoretical yield as its name says is the yield expected, however, many times the difference between the theoretical yield and the actual yield is notorious.
We are given that:
Now, to calculate the percent yield, we need to divide the actual yield by the theoretical and multiply it by 100.
So, calculating we have:
Hence, we have that the percent yield of the reaction is 32.45%.
Have a nice day!
Answer: 323.61 g of will be produced
Explanation:
The given balanced chemical reaction is :
According to stoichiometry :
2 moles of require 1 mole of
Thus 3.00 moles of will require=
of
Thus is the limiting reagent as it limits the formation of product.
As 2 moles of give = 2 moles of
Thus 3.00 moles of give =
of
Mass of
Thus 323.61 g of will be produced from the given moles of both reactants.