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anastassius [24]
3 years ago
5

What happens as a liquid freezes?

Chemistry
1 answer:
marishachu [46]3 years ago
3 0

Answer:

A

Explanation:

When molecules speed up, they become excited and create friction that is transformed into heat, do when an abject cools, the molecules slow down and thus for have less friction.

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What is the molarity of 53.0 grams of HCl dissolved in 400.0 mL of water
Bond [772]

Answer:

Molarity = 3.625 M

Explanation:

Given data:

Mass of HCl = 53.0 g

Volume of water = 400.0 mL (400/1000 = 0.4 L)

Molarity of solution = ?

Solution:

Number of moles of of HCl:

Number of moles = mass/ molar mass

Number of moles = 53 g/ 36.5 g/mol

Number of moles =1.45 mol

Molarity:

Molarity = number of moles of solute / volume of solution in L

Molarity =  1.45 mol / 0.4L

Molarity = 3.625 M

8 0
3 years ago
What is the mass in grams of 5.50 mol of sodium?
Zolol [24]

Answer:

126.5g

Explanation:

n=<u>m</u><u> </u>

M

where n is moles

m is mass of substance

M is molar mass

molar mass of sodium is 23g/mol

m=nM

m=5.5(23)

m=126.5

8 0
3 years ago
Is pentacosane a molecular compound?
jekas [21]

Answer:

Yes

Explanation:

A molecular compound is that one which is composed of molecules formed by atoms of two or different elements. A pentacosane is an alkaline made of unbranched chain of 25 carbons atoms. It has applications in plant metabolite. The molecular formula of pentacosane is C₂₅H₅₂

7 0
3 years ago
Does anyone have the answer sheet for all of Cell energy cycle gizmo part c?
FinnZ [79.3K]

Answer:

No but i wish

Explanation:

7 0
3 years ago
What is the volume of 0.640 grams of Oz gas at Standard Temperature and Pressure (STP)?
Ilia_Sergeevich [38]

Answer: The volume of 0.640 grams of O_{2} gas at Standard Temperature and Pressure (STP) is 0.449 L.

Explanation:

Given: Mass of O_{2} gas = 0.640 g

Pressure = 1.0 atm

Temperature = 273 K

As number of moles is the mass of substance divided by its molar mass.

So, moles of O_{2} (molar mass = 32.0 g/mol) is as follows.

No. of moles = \frac{mass}{molar mass}\\= \frac{0.640 g}{32.0 g/mol}\\= 0.02 mol

Now, ideal gas equation is used to calculate the volume as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

PV = nRT\\1.0 atm \times V = 0.02 mol \times 0.0821 L atm/mol K \times 273 K\\V = 0.449 L

Thus, we can conclude that the volume of 0.640 grams of O_{2} gas at Standard Temperature and Pressure (STP) is 0.449 L.

6 0
3 years ago
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