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3 years ago

7

Mixture A was made by mixing different components together, but it appears to have one phase. Which term best categorizes mixtur

e A?

1 answer:

qwelly [4]3 years ago

6 0

It's a solution. Fjfjdjdjxjdkfjfjdjx

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What is inorganic chemistry.

Oksi-84 [34.3K]

Answer:the branch of chemistry that deals with inorganic compounds

Explanation:

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4 years ago

Which point on the number line represents -3/4

Novosadov [1.4K]

Answer: - 0.75

Explanation:

For this question, you must remember that a fraction can be written of division.

So, -3/4 = -0.75, between -0.7 and -0.8 on the number line.

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3 years ago

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All bodies of water make up a earth's

Delvig [45]

Hey there!

The answer is C, hydrosphere.

The prefix "hydro" means water.

"Sphere" relates to Earth.

The asthenosphere and lithosphere are parts of the crust and mantle of the earth.

The atmosphere is the gases that surround the planet.

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4 years ago

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In the laboratory, a general chemistry student measured the pH of a 0.529 M aqueous solution of phenol (a weak acid), C6H5OH to

Artyom0805 [142]

Answer:

The dissociation constant of phenol from given information is $9.34\times 10^{-11}$ .

Explanation:

The measured pH of the solution = 5.153

$C_6H_5OH\rightarrow C_6H_5O^-+H^+$

Initially c

At eq'm c-x x x

The expression of dissociation constant is given as:

$K_a=\frac{[C_6H_5O^-][H^+]}{[C_6H_5OOH]}$

Concentration of phenoxide ions and hydrogen ions are equal to x.

$pH=-\log[x]$

$5.153=-\log[x]$

$x=7.03\times 10^{-6} M$

$K_a=\frac{x\times x}{(c-x)}=\frac{x^2}{(c-x)}=\frac{(7.03\times 10^{-6} M)^2}{ 0.529 M-7.03\times 10^{-6} M}$

$K_a=9.34\times 10^{-11}$

The dissociation constant of phenol from given information is $9.34\times 10^{-11}$ .

4 0

4 years ago

20.1 g of aluminum and 219 g of chlorine gas react until all of the aluminum metal has been converted to AlCl3. The balanced equ

Romashka-Z-Leto [24]

Answer:

<em>The amount of Cl2 gas left , after the reaction goes to completion is : </em><u><em>139.655 grams</em></u>

Explanation:

Molar mass : It is the mass in grams present in one mole of the substance.

Moles of the substance is calculated by:

$Moles=\frac{Mass}{Molar\ mass}$

$2Al(s)+3Cl_{2}(g)\leftarrow 2AlCl_{3}(g)$

According to this equation:

2 mole of Al = 3 mole of Cl2 = 2 mole of AlCl3

Molar mass of Al = 27.0 g/mol

Mass of Al = 20.1 gram

Moles of Al present in the reaction :

$Moles=\frac{Mass}{Molar\ mass}$

$Moles=\frac{20.1}{26.98}$

Moles of Al = 0.744

Similarly calculate the moles of Cl2

Molar mass of Cl2 = 71.0 g/mol

Mass = 219 gram

$Moles=\frac{Mass}{Molar\ mass}$

$Moles=\frac{219}{70.98}$

Moles of Cl2 = 3.08 moles

According to equation,

2 mole of Al reacts with = 3 mole of Cl2

1 moles of Al reacts with = 3/2 mole of Cl2

0.744 moles of Al reacts with = 3/2(0.744) moles of Cl2

= 1.116 moles of Cl2

But actually present Cl2 = 3.08 moles

Hence Al is the limiting reagent , and Cl2 is the excess reagent.

The whole Aluminium Al get consumed during the reaction.

The amount of Cl2 in excess = Total Cl2 - Cl2 consumed

Cl2 in excess = 3.08 - 1.116 = 1.964 moles

<u>Cl2 in grams</u><u> </u>= 1.964 x 70.90 <u>= 139.655 grams</u>

6 0

4 years ago