Answer:
Calcium oxide: CaO
Copper (II) nitrate: Cu(NO₃)₂
Ammonium chloride: NH₄Cl
Magnesium sulfate: MgSO₄
Copper (I) oxide: Cu₂O
Calcium chloride: CaCl₂
Explanation:
Hello there!
In this case, according the IUPAC rules for naming this inorganic salts, whereas calcium, copper (II), ammonium, magnesium and copper (I) are the cations and oxide, nitrate, chloride and sulfate are the anions, we proceed as follows:
Calcium oxide: CaO
Copper (II) nitrate: Cu(NO₃)₂
Ammonium chloride: NH₄Cl
Magnesium sulfate: MgSO₄
Copper (I) oxide: Cu₂O
Calcium chloride: CaCl₂
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Answer:
The natural abundance of Re-185 is 40% and of Re-187 is 60%
Explanation:
Relative atomic mass is defined as the sum of the mass of each isotope times its relative abundances.
Is Rhenium has only 2 isotopes and the abundances are X and Y we can write:
X + Y = 1 <em>(1)</em>
And:
185X + 187Y = 186.2 <em>(2)</em>
<em>Where X is abundance of Re-185 and Y abundance of Re-187</em>
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Replacing (1) in (2):
185X + 187(1-X) = 186.2
185X + 187-187X = 186.2
-2X = -0.8
X = 0.4 = 40%
And Y = 100% - 40% = 60%
<h3>The natural abundance of Re-185 is 40% and of Re-187 is 60%</h3>
Answer is: mass of iron(II) sulfate pentahydrate (FeSO₄ · 5H₂O) would be 79,62 g.
m(FeSO₄) = 50,0 g.
m(FeSO₄ · 5H₂O) = ?
m(FeSO₄) : M(FeSO₄) = m(FeSO₄ · 5H₂O) : M(FeSO₄ · 5H₂O).
50 g : 151,9 g/mol = m(FeSO₄ · 5H₂O) : 241,9 g/mol.
m(FeSO₄ · 5H₂O) = 50 g · 241,9 g/mol ÷ 151,9 g/mol.
m(FeSO₄ · 5H₂O) = 79,62 g.
M - molar mass.
Answer:
5.450 mol Si₃N₄
Explanation:
Step 1: Write the balanced equation
3 Si + 2 N₂ ⇒ Si₃N₄
Step 2: Establish the theoretical molar ratio between the reactants
The theoretical molar ratio of Si to N₂ is 3:2 = 1.5:1.
Step 3: Establish the experimental molar ratio between the reactants
The experimental molar ratio of Si to N₂ is 16.35:11.26 = 1.45:1. Comparing both molar ratios, we can see that Si is the limiting reactant.
Step 4: Calculate the moles of Si₃N₄ produced from 16.35 moles of Si
The molar ratio of Si to Si₃N₄ is 3:1.
16.35 mol Si × 1 mol Si₃N₄/3 mol Si = 5.450 mol Si₃N₄
