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sp2606 [1]
2 years ago
7

Physical reactions of carbonyl group​

Chemistry
1 answer:
docker41 [41]2 years ago
8 0

Answer:

The polarity of the carbonyl group notably affects the physical properties of melting point and boiling point, solubility, and dipole moment. Hydrocarbons, compounds consisting of only the elements hydrogen and carbon, are essentially nonpolar and thus have low melting and boiling points.

Explanation:

pls mark brainliest and these are my notes from last year.

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g A microwave oven heats by radiating food with microwave radiation, which is absorbed by the food and converted to heat. If the
Sliva [168]

Answer:

The total photons required = 5.19 × 10²⁸ photons

Explanation:

Given that:

the radiation wavelength λ= 12.5 cm = 0.125 m

Volume of the container = 0.250 L = 250 mL

The density of water = 1 g/mL

Density = mass /volume

Mass =  Volume ×  Density

Thus; the mass of the water =  250 mL ×  1 g/mL

the mass of the water = 250 g

the specific heat of water s = 4.18 J/g° C

the initial temperature T_1 = 20.0° C

the final temperature T_2 = 99° C

Change in temperature \Delta T = (99-20)° C = 79 ° C

The heat q absorbed during the process = ms \Delta T

The heat q absorbed during the process = 250 g × 4.18 J/g° C × 79° C

The heat q absorbed during the process = 82555 J

The energy of a photon can be represented by the equation :

= hc/λ

where;

h = planck's constant = 6.626 \times 10^{-34} \ J.s

c = velocity of light = 3.0 \times 10^8 \ m/s

=  \dfrac{6.626 \times 10^{-34} \times 3.0 \times 10^8}{0.125}

= 1.59024 \times 10^{-24} J

The total photons required = Total heat energy/ Energy of a photon

The total photons required = \dfrac{82555 J}{1.59024 \times 10^{-24}J}

The total photons required = 5.19 × 10²⁸ photons

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3 years ago
What uses lines of bubbles in a superheated liquid to track particles?
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6 0
2 years ago
A gas occupying a volume of 656.0 mL at a pressure of 0.884 atm is allowed to expand at constant temperature until its pressure
7nadin3 [17]

Answer:

1.14 × 10³ mL

Explanation:

Step 1: Given data

  • Initial volume of the gas (V₁): 656.0 mL
  • Initial pressure of the gas (P₁): 0.884 atm
  • Final volume of the gas (V₂): ?
  • Final pressure of the gas (P₂): 0.510 atm

Step 2: Calculate the final volume of the gas

If we assume ideal behavior, we can calculate the final volume of the gas using Boyle's law.

P₁ × V₁ = P₂ × V₂

V₂ = P₁ × V₁/P₂

V₂ = 0.884 atm × 656.0 mL/0.510 atm = 1.14 × 10³ mL

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2 years ago
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