One isomer is formed
1,1- Dichloroethane is the isomer.
If another hydrogen of c2h5cl is replaced by a chlorine atom to yield c2h4cl2, it would result in one isomer.
- In contrast to 1,2-dichloroethane, which has two chlorine atoms connected to distinct carbon atoms, 1,1-dichloroethane has two chlorine atoms bound to the same carbon atom.
- Isomers are each of two or more compounds having the same formula but various atom arrangements in the molecule and unique characteristics.
<h3>What three types of isomers are there?</h3>
- Chain isomers
- Functional group isomers
- Positional isomers
These are the three different categories of structural isomers.
<h3>How is an isomer recognized?</h3>
- Their bonding patterns and the way they occupy three-dimensional space can be used to distinguish them.
- Determine the bonding patterns of structural (constitutional) isomers.
- Although the atoms in the compounds are the same, their connections create various functional groups.
<h3>What makes isomers significant?</h3>
- Because two isomers might have the same chemical formula but different chemical structures, they are significant.
- The molecule's properties are influenced by its structure.
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The balanced equation between NaOH and H₂SO₄ is as follows
2NaOH + H₂SO₄ ---> Na₂SO₄ + 2H₂O
stoichiometry of NaOH to H₂SO₄ is 2:1
number of moles of NaOH moles reacted = molarity of NaOH x volume
number of NaOH moles = 0.08964 mol/L x 27.86 x 10⁻³ L = 2.497 x 10⁻³ mol
according to molar ratio of 2:1
2 mol of NaOH reacts with 1 mol of H₂SO₄
therefore 2.497 x 10⁻³ mol of NaOH reacts with - 1/2 x 2.497 x 10⁻³ mol of H₂SO₄
number of moles of H₂SO₄ reacted - 1.249 x 10⁻³ mol
Number of H₂SO₄ moles in 34.53 mL - 1.249 x 10⁻³ mol
number of H₂SO₄ moles in 1000 mL - 1.249 x 10⁻³ mol / 34.53 x 10⁻³ L = 0.03617 mol
molarity of H₂SO₄ is 0.03617 M
The volume of 0. 250 mole sample of 
gas occupy if it had a pressure of 1. 70 atm and a temperature of 35 °C is 3.71 L.
Calculation,
According to ideal gas equation which is known as ideal gas law,
PV =n RT
- P is the pressure of the hydrogen gas = 1.7 atm
- Vis the volume of the hydrogen gas = ?
- n is the number of the hydrogen gas = 0.25 mole
- R is the universal gas constant = 0.082 atm L/mole K
- T is the temperature of the sample = 35°C = 35 + 273 = 308 K
By putting all the values of the given data like pressure temperature universal gas constant and number of moles in equation (i) we get ,
1.7 atm×V = 0.25 mole ×0.082 × 208 K
V = 0.25 mole ×0.082atm L /mole K × 308 K /1.7 atm
V = 3.71 L
So, volume of the sample of the hydrogen gas occupy is 3.71 L.
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Here you go:
Continent Polar - Cold and Dry
Maritime Polar - Cold and Humid
Arctic - Extremely Cold and Dry
Maritime Tropical- Warm and Humid
Hope this helps:)
