Explanation:
When we move across a period from left to right then there will occur an increase in electronegativity and also there will occur an increase in non-metallic character of the elements.
As sulfur (S) is a group 16 element and chlorine (Cl) is a group 17 element. Hence, sulfur (S) is more metallic in nature than chlorine.
This means that chlorine (S) is less metallic than chlorine (Cl).
Both indium (I) and aluminium (Al) are group 13 elements. And, when we move down a group then there occur an increase in non-metallic character of the elements. As indium belongs to group 13 and period 5 whereas aluminium belongs to group 13 and period 3.
Therefore, aluminium (Al) is more metallic than indium (In).
Arsenic (Ar) is a group 15 element and bromine (Br) is a group 17 element. Therefore, arsenic is more metallic than bromine.
I don’t know but I think it would be products... that’s the best I can give. I’ll look more into it
That's a compound
The Cu stands for Copper, and the O stands for oxygen
The enthalpy of the change of the reaction P₄O₆ + 2O₂ ------ P₄O₁₀ is -1300.1kJ.
The reactions are as follows:
P₄O₆ + 2O₂ ------> P₄O₁₀
P₄ + 3O₂ ------->P₄O₆
Here, ΔHₐ = -1640.1kJ
P₄ + 5O₂ --------> P₄O₁₀
Here, ΔHₓ = -2940.1kJ
The enthalpy change of any type of reaction depends on the initial and final states of the reactions and is independent of the path taken by the system to reach the product.
To find the overall change in enthalpy, we need to sum up the reactions at each stage. On reversing the reactions we get,
P₄O₆ ------> P₄ + 3O₂.................(1)
Here, ΔHₐ = +1640.1kJ
P₄O₁₀------> P₄ + 5O₂.................(2)
Here, ΔHₓ = -2940.1kJ
By adding (1) and (2) we get,
P₄O₆ + 2O₂ ------> P₄O₁₀
By reversing (1) the sign of the enthalpy is changed. The enthalpy is given by
ΔH = ΔHₐ + ΔHₓ
ΔH = 1640.1 + (-2940.1)
ΔH = -1300.1kJ
Therefore the enthalpy of the reaction, P₄O₆ + 2O₂ ------> P₄O₁₀ is -1300.1kJ
To know more about entropy, click below:
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Tin is Sn^2+
Chlorine is Cl^1-