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3 years ago

What would the product look like if ROOR weren't used?

Chemistry

1 answer:

S_A_V [24]3 years ago

4 0

Answer:

The least substituted product (anti-Markovnikov)

Explanation:

The ROOR is used in the addition reaction of HBr to an organic substance (an alkene for example).

In normal conditions (with no ROOR) the adition of the halogen will be performed in the most substituted C (following the rule of Markovnikov that says that the stability increases with the more substituted is the C).

But in presence of ROOR, the reaction takes other mechanism (free radicals), and the product in this case is the one with the Br added in the least substituted C.

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If you have an altitude of 55 mi. (miles), which layer of the atmosphere are you in?

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2 years ago

What is the molarity of a solution in which 25g NaCl in a 2.00 L solution?

Paladinen [302]

Mass of sodium :- 23 grams

Mass of Chlorine :- 35.5 grams

Mass of NaCl :- 58.5 grams

mass given :- 25 grams

moles :- 0.432 ( given mass/ ionic mass)

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3 years ago

Suppose of nickel(II) chloride is dissolved in of a aqueous solution of potassium carbonate. Calculate the final molarity of chl

stich3 [128]

Answer: Molarity of chloride anion = 0.32 M

Note: the question is missing some values. The full question is given below;

Suppose 7.26 g of nickel(II) chloride is dissolved in 350 mL of a 0.50 M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits.

Explanation:

Molarity or molar concentration is the number of moles (mol) of component per volume (liters) concentration of solution in mol/L or M

The mass of nickel (II) chloride is 7.26 g.

The volume of potassium carbonate is 350 mL = 0.35 L

The molarity of potassium carbonate solution is 0.50 M

The reaction of nickel (II) chloride and potassium carbonate is given below.

NiCl₂(aq) + KCO₃(aq) --------> KCl(aq) +NiCO₃(s)

The dissociation of nickel (II) chloride is given below.

NiCl₂ -----> Ni²⁺ + 2Cl⁻

The molar mass of nickel (II) chloride is 129.6 g/mol

The moles of nickel (II) chloride can be calculated by the formula given below;

No of moles = mass(g) / molar mass (g/mol)

No of moles = 7.26 / 129.6 = 0.056 moles

Therefore, molarity of NiCl₂ = 0.056 moles/ 0.35 L = 0.16 M

The molarity of 1 mole nickel (ii) chloride is 0.16 m and according to dissociation of nickel (II) chloride, 1 mole of nickel (II) chloride gives 2 moles of chloride anion.

Therefore, the molarity of chloride anion = 0.16 * 2 = 0.32 M

3 0

3 years ago

The part of an atom where nearly whole mass is concentrated is called

qwelly [4]

Answer:

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3 years ago

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