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vova2212 [387]
2 years ago
7

Help this is due in 5 minutes

Chemistry
2 answers:
Fed [463]2 years ago
6 0

Answer:

no

Explanation:

they avoid most fur and bones because hawks and eagles rip them apart to get the flesh and owls swallow bones and fur too

stepan [7]2 years ago
4 0
Give me brainliest just cause I’m smart and also no
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What is the energy of light with a wavelength of 468 nm? (The speed of light
marshall27 [118]

The answer for the problem is explained below.

The option for the answer is "D".

<u><em>Therefore the energy of the light is  4.25 × 10^-19 J</em></u>

Explanation:

Given:

wavelength (λ) = 468 nm = 468×10^-9 m

speed of light (c) = 3.00 x 10^8m/s

Planck's constant is 6.626 x 10^-34J·s

To solve:

energy of light (E)

We know,

E =(h×c) ÷ λ

E = ( 6.626 x 10^-34 ×  3.00 x 10^8) ÷ 468×10^-9

E = 4.25 × 10^-19 J

<u><em>Therefore the energy of the light is  4.25 × 10^-19 J</em></u>

6 0
2 years ago
The pyrolysis of ethane proceeds with an activation energy of about 300 kJ/mol. How much faster is the decomposition at 625°C th
Alona [7]

Answer:

The decomposition of ethane is 153.344 times much faster at 625°C than at 525°C.

Explanation:

According to the Arrhenius equation,

K=A\times e^{\frac{-Ea}{RT}}

\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]

where,

K_2 = rate of reaction at T_2

K_1 = rate of reaction at T_1

Ea = activation energy of the reaction

R = gas constant = 8.314 J/K mol

E_a=300 kJ/mol=300,000 J/mol

T_2=625^oC=898.15 K,T_1=525^oC=798.15 K

\log (\frac{K_2}{K_1})=\frac{300,000 J/mol}{2.303\times 8.314 J/K mol}[\frac{1}{798.15 K}-\frac{1}{898.15 K}]

\log (\frac{K_2}{K_1})=2.185666

K_2=153.344\times K_1

The decomposition of ethane is 153.344 times much faster at 625°C than at 525°C.

4 0
3 years ago
What is the three properties of matter
Sav [38]
A solid, a liquid or a gas.
6 0
3 years ago
Read 2 more answers
Use the reaction given below to solve the problem that follows: Calculate the mass in grams of aluminum oxide produced by the re
bearhunter [10]

Answer:  28.4 g of aluminum oxide is produced by the reaction of 15.0 g of aluminum metal

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}   

\text{Moles of} Al=\frac{15.0g}{27g/mol}=0.556moles

The balanced chemical equuation is:

4Al+3O_2\rightarrow 2Al_2O_3  

According to stoichiometry :

4 moles of Al produce == 2 moles of Al_2O_3

Thus 0.556 moles of Al will produce=\frac{2}{4}\times 0.556=0.278moles  of Al_2O_3

Mass of Al_2O_3=moles\times {\text {Molar mass}}=0.278moles\times 102g/mol=28.4g

Thus 28.4 g of aluminum oxide is produced by the reaction of 15.0 g of aluminum metal.

7 0
2 years ago
Suppose you have a mixture of copper sulfate (CuSO4) and azulene (C10H8, you may wish to know the structure of azulene). Both co
iVinArrow [24]

Answer:

Aqueous layer (1 M HCI)

Explanation:

First of us I want to remind you of the cliché in chemistry that like dissolves like. In solvent extraction, a mixture is dissolved in a system consisting of two immiscible solvents. One layer is organic while the other layer is aqueous.

Polar substances partition in the aqueous layer while nonpolar substances partition in the organic layer.

Since Copper sulfate is ionic, we will find it in the aqueous layer according to the old chemistry cliche.

3 0
3 years ago
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