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ra1l [238]
3 years ago
15

Which scientist established the law of octaves ?

Chemistry
2 answers:
quester [9]3 years ago
8 0

Answer:

John Newlands

Explanation:

just did on edgen

goblinko [34]3 years ago
5 0

the answer is D. John Newlands <3

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2. What is the total mass of Chlorine in ZnCl,?
Vedmedyk [2.9K]

Answer:

35.5

Explanation:

35.5.

relative moleculer mass

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2 years ago
Why is making a peanut pretzel and cereal mixture
guajiro [1.7K]
It is two or more objects and different things that can be removed from each other.
7 0
2 years ago
Draw the structure of 4-methyl-5-oxohexanal.
aniked [119]

Answer:

Explanation:

The structural formula provides more information which is often used to represent a particular organic substance. A structural formula indicates how the atoms are arranged within the molecule of a substance. From the information, the structure of  4-methyl-5-oxohexanal is represented by using a stick formula where the methyl group falls into position 4 and oxygen group falls into position 5 on the hexanal compound.

The structure is provided in the image attached below for better understanding.

4 0
3 years ago
Convert 1.39 x 10^24 atoms of carbon to moles of carbon
Nimfa-mama [501]
If 1mol ------- is ----------- 6,02×10²³
so x     ------- is ----------- 1,39×10²⁴

x=\frac{1,39*10^{24}*1mol}{6,02*10^{23}}\approx2,31mol
8 0
3 years ago
Read 2 more answers
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O 3 ( g ) + NO ( g )
Aleksandr [31]

Answer:

(a) 7.11x10⁻⁴ M/s

(b) 2.56 mol.L⁻¹.h⁻¹

Explanation:

(a) The reaction is:

O₃(g) + NO(g) → O₂(g) + NO₂(g)   (1)

The reaction rate of equation (1) is given by:

rate = k*[O_{3}][NO]     (2)

<u>We have:</u>

k: is the rate constant of reaction = 3.91x10⁶ M⁻¹.s⁻¹

[O₃]₀ = 2.35x10⁻⁶ M

[NO]₀ = 7.74x10⁻⁵ M

Hence, to find the inital reacion rate we will use equation (2):

rate = k*[O_{3}]_{0}[NO]_{0} = 3.91 \cdot 10^{6} M^{-1}s^{-1}*2.35\cdot 10^{-6} M*7.74 \cdot 10^{-5} M = 7.11 \cdot 10^{-4} M/s  

Therefore, the inital reaction rate is 7.11x10⁻⁴ M/s

(b) The number of moles of NO₂(g) produced per hour per liter of air is:

t = 1 h

V = 1 L

\frac{\Delta[NO_{2}]}{\Delta t} = rate

\frac{\Delta[NO_{2}]}{\Delta t} = 7.11 \cdot 10^{-4} M/s*\frac{3600 s}{1 h} = 2.56 mol.L^{-1}.h{-1}

Hence, the number of moles of NO₂(g) produced per hour per liter of air is 2.56 mol.L⁻¹.h⁻¹

I hope it helps you!                                

5 0
2 years ago
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