Answer:
The answer to your question is below
Explanation:
1.- It is a metal attach to an oxygen, then the name would be name of the metal + oxide.
Zinc oxide
2.- It is a metal attach to a non metal, then the name would be name of the metal + name of the non metal ending in "ide".
Manganese phosphide
3.- it is also a metal attach to a non metal, then the name would be name of the metal + name of the non metal with ending "ide".
Calcium phosphide
4.- K₂S
5.- PbBr₄
6.- Ba₃N₂
Answer:
A for 1 and 4 B for 2 and 3 ..........
Answer:
Heat, Q = 262 kJ
Explanation:
Given that,
Mass of a sample, m = 750 g
Initial temperature,
Final temperature,
The specific heat of the sample,
We need to find the amount of heat released. The amount of heat released is given by the formula as follows :
So, 262 kJ of heat is released by the sample.
the equilibrium concentration of H₂(g) at 700°C = 0.00193 mol/L
0.00193 mol/L
Given that:
numbers of moles of H₂S = 0.59 moles
Volume = 3.0-L
Equilibrium constant = 9.30 × 10⁻⁸
The equation for the reaction is given as :
2H₂S ⇄ 2H₂(g) + S₂(g)
The initial concentration of H₂S =
The initial concentration of H₂S =
= 0.1966 mol/L
The ICE table is shown be as :
2H₂S ⇄ 2H₂(g) + S₂(g)
Initial 0.9166 0 0
Change -2 x +2 x + x
Equilibrium (0.9166 - 2x) 2x x
(since 2x < 0.1966 if solved through quadratic equation)
The equilibrium concentration for H₂(g) = 2x
∴
= 0.00193 mol/L
Thus, the equilibrium concentration of H₂(g) at 700°C = 0.00193 mol/L
To know more about equilibrium concentration
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Hey there!
I believe the correct answer is B. Grasses
Hope this helps you!
God bless ❤️
xXxGolferGirlxXx