Answer:
131.5 kJ
Explanation:
Let's consider the following reaction.
CaCO₃(s) → CaO(s) + CO₂(g)
First, we will calculate the standard enthalpy of the reaction (ΔH°).
ΔH° = 1 mol × ΔH°f(CaO(s)) + 1 mol × ΔH°f(CO₂(g)
) - 1 mol × ΔH°f(CaCO₃(s)
)
ΔH° = 1 mol × (-634.9 kJ/mol) + 1 mol × (-393.5 kJ/mol) - 1 mol × (-1207.6 kJ/mol)
ΔH° = 179.2 kJ
Then, we calculate the standard entropy of the reaction (ΔS°).
ΔS° = 1 mol × S°(CaO(s)) + 1 mol × S°(CO₂(g)
) - 1 mol × S°(CaCO₃(s)
)
ΔS° = 1 mol × (38.1 J/mol.K) + 1 mol × (213.8 J/mol.K) - 1 mol × (91.7 J/mol.K)
ΔS° = 160.2 J/K = 0.1602 kJ/K
Finally, we calculate the standard Gibbs free energy of the reaction at T = 25°C = 298 K.
ΔG° = ΔH° - T × ΔS°
ΔG° = 179.2 kJ - 298 K × 0.1602 kJ/K
ΔG° = 131.5 kJ
I believe the correct answer from the choices listed above is option D. Catalysts lower the activation energy of a chemical reaction. It <span>is a substance which speeds up a reaction, but is chemically unchanged at the end of the reaction. It provides another pathway for the reaction to occur.</span>
Hello!
According to the
Charles' Law, the volume of a gas is proportional to temperature when pressure is constant. When going from New York to Florida, if the pressure is left constant
the volume of the tires will increase.The final volume of the tires can be calculated from the following equation, derived from Charles' Law:
Have a nice day!
Answer:There are important differences between naturally occurring sugars, ... Understanding these differences can help you make choices that are better for your health. ... of energy, along with a bevy of vitamins, minerals, and phytonutrients. ... sugar substitutes, but many people find they have an unpleasant
Explanation:
Answer:
- <u><em>You should expect that the ionic bond in LiBr is stronger than the bond in KBr.</em></u>
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Explanation:
The<em> ionic bonds</em> are formed by the electrostatic attraction between the ions, cations and anions.
In KBr the cation is K⁺ and the anion is Br⁻.
In LiBr the cation is Li⁺ and the anion is Br⁻.
You must expect that the bond strength depends mainly on the charges present on each ion and the distance between them.
Nevertheless, the effect of the distance between the radius dominate the trendency of the bond strength, which makes that the ionic strength trend be related to the ionic radius trend.
Lithium is a smaller ion than Potassium (both are in the same group and Lithium is above Potassium).
Thus, you should expect that the Li ion is closer to the Br ion than what the K ion is to the Br ion and expect that the bond between a Li ion and the Br ion be stronger than the bond between the K ion and the Br ion.
