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AlekseyPX
3 years ago
12

A beaker contains 500 ml of 2.40M KNO3 the beaker is left uncovered so that all of the water evaporates. What mass of KNO3 cryst

als will remain in the beaker when the beaker is dry.
Chemistry
1 answer:
telo118 [61]3 years ago
6 0

Answer:

242.4 g

Explanation:

RAM of KNO3=39+14+(16×3)=101

Mass=morality×RAM

101*2.4=242.4

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During electrophilic aromatic substitution, a resonance-stabilized cation intermediate is formed. Groups, already present on the
DIA [1.3K]

Answer:

See explanation and image attached

Explanation:

Aromatic compounds undergo electrophilic aromatic substitution reactions in which the aromatic ring is maintained.

Substituted benzenes may be more or less reactive towards electrophilic aromatic substitution than benzene depending on the nature of the substituent present in the ring.

Substituents that activate the ring towards electrophilic substitution such as -OCH3 are ortho-para directing.

The major products of the bromination of anisole are p-bromoanisole and o-bromoanisole. The resonance structures leading to these products are shown in the image attached.

5 0
3 years ago
Does anyone know how to fill in this diagram?
tangare [24]

Answer:

solid to gas is sublimation

gas to solid is deposition

liquid to gas is evaporation/boiling

the rest are correct

3 0
3 years ago
What mass of solute should you measure out in order to make 1,000 mL of a 0.3 M solution of magnesium phosphate Mg3(PO4)2?
vivado [14]

Hey there !

Molecular Weight: 262.86 g/mol

Volume in liters : 1,000 mL => 1,000 / 1000 => 1 L

Number of moles of solution :

number of moles = volume x molarity

number of moles = 1 x 0.3  => 0.3 moles

Therefore:

1 mole Mg₃(PO₄)₂ ------------------- 262.86 g

0.3 moles ----------------------------- mass of Mg₃(PO₄)₂  ??

mass of Mg₃(PO₄)₂ = 0.3 x 262.86 / 1

mass of Mg(PO₄)₂ => 78.858 g

Hope this helps!

7 0
2 years ago
Calculate the ph of 0,24 m of kch3coo.? ​
Galina-37 [17]

Answer:

Correct option is A)

[H

+

]=

KaC

=

1.8×10

−6

=1.34×10

−3

pH=−log[H

+

]

=2.88

Explanation:

here is your answer if you like my answer please follow

6 0
3 years ago
How many total atoms are in 0.560 g of P2O5
ioda

Answer:

16.499 × 10∧ 21 atoms

Explanation:

Given data:

mass of P2O5= 0.560 g

number of atoms= ?

first of all we will calculate the molar mass of P2O5:

P = 2×31 g/mol = 62 g/mol

O = 5× 16 = 80 g/mol

molar mass of P2O5 = 142 g/mol

Noe we will find the moles of 0.560 g P2O5:

moles = mass / molar mass

moles = 0.560 g/ 142 g/mol

moles = 0.0039 mol

now we will find the atoms present in 0.0039 moles:

0.0039 × 6.02 × 10∧ 23 molecules

2.357 × 10∧ 21 molecules

P2O5 consist of 7 atoms:

2.357 × 10∧ 21  × 7 = 16.499 × 10∧ 21 atoms

7 0
3 years ago
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