Answer:
76.0%
Explanation:
Let's consider the following reaction.
CaCO₃(s) ⇄ CaO(s) + CO₂(g)
At equilibrium, the equilibrium constant Kp is:
Kp = 1.16 = pCO₂ ⇒ pCO₂ = 1.16 atm
We can calculate the moles of CO₂ at equilibrium using the ideal gas equation.
From the balanced equation, we know that 1 mole of CO₂ is produced by 1 mole of CaCO₃. Taking into account that the molar mass of CaCO₃ is 100.09 g/mol, the mass of CaCO₃ that reacted is:
The percentage by mass of the CaCO₃ that reacted to reach equilibrium is:
If you were to compare the mass of the products and reactants in a reaction, you would find that the mass of the products is <span>equal to the mass of the reactants.</span>
Answer:
0.962 atm.
97.4 kPa.
731 torr.
14.1 psi.
97,434.6 Pa.
Explanation:
Hello.
In this case, given the available factors equaling 1 atm of pressure, each required pressure turns out:
- Atmospheres: 1 atm = 760 mmHg:
- Kilopascals:: 101.3 kPa = 760 mmHg:
- Torrs: 760 torr = 760 mmHg:
- Pounds per square inch: 14.69 psi = 760 mmHg:
- Pascals: 101300 Pa = 760 mmHg:
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