Answer:
2Ag(s) + 1H2S(g) → 1Ag2S(s) + 1H2(g)
Explanation:
Step 1: Data given
Ag(s) + H2S(g) → Ag,S(s) + H2(g)
Ag has and oxidation number of +1
S has an oxidation number of -2
H has an oxidation number of +1
Step 2: The balanced equation
Ag+ + 2H+ + S^2- →
The silver ion and the sulfur ion will bind, but we need 2 silver atoms to bind with 1 sulfur atom.
2 H- atoms will appear as H2.
The balanced equation is:
2Ag+ + 2H+ +S^2- → Ag2S + H2
2Ag(s) + 1H2S(g) → 1Ag2S(s) + 1H2(g)
Ionization Trend: First ionization energy will increase left to right across a period and increase bottom to top of a family (column).
A) Sr, Be, Mg are all in column 2 of the periodic table. Based on the first ionization rule above, from increasing to decreasing energy, the order is: Be, Mg, Sr
B) Bi, Cs, Ba are all in the same row of the periodic table. Based on the first ionization rule above, from increasing to decreasing energy, the order is: Bi, Ba, Cs
C) Same rule as above. Order is: Na, Al, S
The maximum mass of B₄C that can be formed from 2.00 moles of boron (III) oxide is 55.25 grams.
<h3>What is the stoichiometry?</h3>
Stoichiometry of the reaction gives idea about the relative amount of moles of reactants and products present in the given chemical reaction.
Given chemical reaction is:
2B₂O₃ + 7C → B₄C + 6CO
From the stoichiometry of the reaction, it is clear that:
2 moles of B₂O₃ = produces 1 mole of B₄C
Now mass of B₄C will be calculated by using the below equation:
W = (n)(M), where
- n = moles = 1 mole
- M = molar mass = 55.25 g/mole
W = (1)(55.25) = 55.25 g
Hence required mass of B₄C is 55.25 grams.
To know more about stoichiometry, visit the below link:
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The relative molecular mass of the gas : 64 g/mol
<h3>Further explanation</h3>
Given
Helium rate = 4x an unknown gas
Required
The relative molecular mass of the gas
Solution
Graham's Law

r₁=4 x r₂
r₁ = Helium rate
r₂ = unknown gas rate
M₁= relative molecular mass of Helium = 4 g/mol
M₂ = relative molecular mass of the gas
Input the value :

1 Oz is 28.3495 grams
hope this helps!