Answer:
2Fe(s) + 3Cl2(g) → 2FeCl3(s)
Explanation:
Step 1: Data given
iron = Fe = solid = Fe(s)
chlorine = Cl2 = gas = Cl2(g)
iron(III) chloride = FeCl3 = solid = FeCl3(s)
Step 2: The unbalanced equation
Fe(s) + Cl2(g) → FeCl3(s)
Step 3: Balancing the equation
Fe(s) + Cl2(g) → FeCl3(s)
On the left we have 2x Cl (in Cl2) and on the right side we have 3x Cl (in FeCl3). To balance the amount of Cl we have to multiply Cl2 (on the left) by 3 and FeCl3 by 2.
Fe(s) + 3Cl2(g) → 2FeCl3(s)
On the left side we have 1x Fe and on the right side we have 2x Fe (in 2FeCl3). To balance the amount of Fe, we have to multiply Fe on the left side by 2. Now the equation is balanced.
2Fe(s) + 3Cl2(g) → 2FeCl3(s)
Answer: The last electron will be filled in first orbital of 3p sub-shell.
Explanation: Filling of electrons in orbitals is done by using Hund's Rule.
Hund's rule states that the electron will be singly occupied in the orbital of the sub-shell before any orbital is doubly occupied.
For filling up of the electrons in Sulfur atom having 16 electrons. First 10 electrons will completely fill according to Aufbau's Rule in 1s, 2s and 2p sub-shells and last 6 electrons are the valence electrons which will be filled in the order of 3s and then 3p.
3s sub-shell will be fully filled and the orbitals of 3p sub-shell will be first singly occupied and then pairing will take place. Hence, the last electron will be filled in the first orbital of 3p-sub-shell.
Below are I think the data for this problem:
Given the following data:
<span>Ca (s) + 2 C (graphite) → CaC2 (s) ∆H = -62.8 kJ </span>
<span>Ca (s) + ½ O¬2 (g) → CaO (s) ∆H = -635.5 kJ </span>
<span>CaO (s) + H2O (l) → Ca(OH)2 (aq) ∆H = -653.1 kJ </span>
<span>C2H2 (g) + 5/2 O¬2 (g) → 2 CO2 (g) + H2O (l) ∆H = -1300 kJ </span>
<span>C (graphite) + O¬2 (g) → CO2 (g) ∆H = -393.51 kJ
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Below is the answer:
CaC2 (s) + 2 H2O (l) → Ca(OH)2 (aq) + C2H2 (g)
<span>So what you do is: </span>
<span>Times the first equation by -1 Second by 1 Third By 1 Fourth by -1 and Fifth by 2 </span>
<span>So This gives us: </span>
<span>1.CaC2--> Ca+2C </span>
<span>2.Ca+1/2O2-->CaO </span>
<span>3.CaO+H2O-->Ca(OH)2 </span>
<span>4.2CO2+H2O-->C2H2+5/2O2 </span>
<span>5.2C+202-->2CO2 </span>
<span>Now you cancel out like terms on either sides of the equation and you end up with </span>
<span>CaC2 (s) + 2 H2O (l) → Ca(OH)2 (aq) + C2H2 (g) Just what you wanted </span>
<span>So to calculate ∆H: </span>
<span>62.8-635.5-653.1+1300-787.02= -712.82</span>
Step 1 : Write balanced chemical equation.
CaF₂ can be converted to F₂ in 2 steps. The reactions are mentioned below.
I] 
II] 
The final balanced equation for this reaction can be written as
Step 2: Find moles of CaF₂ Using balanced equation
We have 1.12 mol F₂
The mole ratio of CaF₂ and F₂ is 1:1
Step 3 : Calculate molar mass of CaF2.
Molar mass of CaF₂ can be calculated by adding atomic masses of Ca and F
Molar mass of CaF₂ = Ca + 2 (F)
Molar mass of CaF₂ = 40.08 + 18.998 = 78.08 g
Step 4 : Find grams of CaF₂
Grams of CaF₂ = 
Grams of CaF₂ = 87.45 g
87.45 grams of CaF2 would be needed to produce 1.12 moles of F2.
A <span> constellations is a collection of stars
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