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4 years ago

Draw the major monobromination product formed by heating the following alkane with bromine.

1 answer:

8 0

A monobromination reaction of an alkane involves an alkane and bromine. The position of the hydrogen atom that will be substituted by the bromine free radical will depend on the order of the alkane. The bromine will attach to the carbon that has the most substituents.

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How do we think that Mars lost atmospheric gas?

grin007 [14]

the rocky planet was exposed to harsh and forceful solar winds, which blew the Martian atmosphere away.

Another option for thickening the atmosphere of Mars, and, in turn, raising the temperature of the planet, would be to set up solar-powered, greenhouse-gas producing factories.

7 0

2 years ago

While hiking in Costa Rica, Bert discovers a new species of arthropod. Which characteristics should he look at to determine in w

alex41 [277]

Answer:

Characteristics outlined below

Explanation:

Anthropods, though they generally possess exoskeleton, segmented bodies and joint appendages, are divided into four (4) groups:

<em>Tracheata</em> (breath through channels in their bodies. E.g. insects)
Chelicerata (More than four legs, one pir of chelicerae i.e. claw or pincer. E.g. Scorpions and spiders)
<em>Crustaceans</em> (Have a large rigid exoskeletal, without a circulatory system. E.g. Shrimps, crabs)
<em>Trilobite</em> (extinct three-headed/lobed marine species)

6 0

4 years ago

What type of substance would be best for use in a cooling system?

Sonbull [250]

Answer:

Explanation:

<h3><em>Liquid with a low specific heat </em></h3>

3 0

3 years ago

At 570. mmHg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a

marusya05 [52]

Answer:

1560 mmHg is the final pressure

Explanation:

To solve this problem we need to apply the Ideal Gases Law Equation:

P . V = n . R . T

First of all, we need to convert the volume to L, T° to Absolute T° (T°C + 273) and pressure from mmHg to atm

570 mmHg . 1atm/760 mmHg = 0.75 atm

25°C + 273 = 298K

175°C + 273 = 448K

2270 mL . 1L/1000mL = 2.27L

1250 mL . 1L/1000mL = 1.25L

P.V = n . R. T is the main equation but in both cases n and R are constant. We can ignore them, so we make this formula for each situation:

P . V / T = n . R → P₁ . V₁ / T₁ = P₂ . V₂ / T₂

We replace data: 0.75 atm . 2.27L / 298K = P₂ . 1.25L / 448K

(0.75 atm . 2.27L / 298K). 448K = P₂ . 1.25L

2.56 atm.L = P₂ . 1.25L → P₂ = 2.56atm.L / 1.25L = 2.05 atm

We finally convert the atm to mmHg to reach the answer

2.05 atm . 760 mmHg / 1atm = 1556 mmHg ≅ 1560 mmHg

3 0

3 years ago

You need to produce a buffer solution that has a pH of 5.50. You already have a solution that contains 10 mmol (millimoles) of a

balandron [24]

Answer:

56.9 mmoles of acetate are required in this buffer

Explanation:

To solve this, we can think in the Henderson Hasselbach equation:

pH = pKa + log ([CH₃COO⁻] / [CH₃COOH])

To make the buffer we know:

CH₃COOH + H₂O ⇄ CH₃COO⁻ + H₃O⁺ Ka

We know that Ka from acetic acid is: 1.8×10⁻⁵

pKa = - log Ka

pKa = 4.74

We replace data:

5.5 = 4.74 + log ([acetate] / 10 mmol)

5.5 - 4.74 = log ([acetate] / 10 mmol)

0.755 = log ([acetate] / 10 mmol)

10⁰'⁷⁵⁵ = ([acetate] / 10 mmol)

5.69 = ([acetate] / 10 mmol)

5.69 . 10 = [acetate] → 56.9 mmoles

6 0

3 years ago