An exergonic reaction is a chemical reaction where the change in the free energy is negative (there is a net release of free energy),[1] indicating a spontaneous reaction. For processes that take place under constant pressure and temperature conditions, the Gibbs free energy is used whereas the Helmholtz energy is used for processes that take place under constant volume and temperature conditions.
Symbolically, the release of free energy, G, in an exergonic reaction (at constant pressure and temperature) is denoted as
{\displaystyle \Delta G=G_{\rm {products}}-G_{\rm {reactants}}<0.\,}
Although exergonic reactions are said to occur spontaneously, this does not imply that the reaction will take place at an observable rate. For instance, the disproportionation of hydrogen peroxide is very slow in the absence of a suitable catalyst. It has been suggested that eager would be a more intuitive term in this context.[2]
More generally, the terms exergonic and endergonic relate to the free energy change in any process, not just chemical reactions. An example of an exergonic reaction is cellular respiration. This relates to the degrees of freedom as a consequence of entropy, the temperature, and the difference in heat released or absorbed.
By contrast, the terms exothermic and endothermic relate to the overall exchange of heat during a process
Answer:
The answer to your question is the limiting reactant is CuSO₄ and 0.975 moles of Cu were obtained
Explanation:
moles of Copper = ?
mass of Aluminum = 29 g
mass of CuSO₄ = 156 g
Limiting reactant = ?
Balanced Chemical reaction
3 CuSO₄ + 2 Al ⇒ 3 Cu + Al₂(SO₄)₃
Calculate the moles of reactants
CuSO₄ = 64 + 32 + (16 x 4) = 160g
Al = 27 g
160 g of CuSO₄ ----------------- 1 mol
156 g ----------------- x
x = (156 x 1) / 160
x = 0.975 moles
27 g of Al -------------------------- 1 mol
29 g of Al -------------------------- x
x = (29 x 1)/27
x = 1.07 moles
Calculate proportions to find the limiting reactant
Theoretical 3 moles CuSO₄/2 moles Al = 1.5 moles
Experimental 0.975 moles CuSO₄/1.07 moles = 0.91
The experimental proportion was lower than the theoretical proportion that means that the limiting reactant is CuSO₄.
3 moles of CuSO₄ ------------------ 3 moles of Cu
0.975 moles of CuSO₄ --------------- x
x = (0.975 x 3)/3
x = 0.975 moles of Cu were obtained.
Sun isn't actually planet but star. Really big ball made of gases. Sun's mass consists of hydrogen (~73%); the rest is mostly helium (~25%). Sun is the biggest object in our Solar System. It's 99.86% of the total mass of the Solar System.
... wikipedia is really grat if you have questions like that ;)
