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Mashutka [201]
3 years ago
12

Choose the biggest number A: 5 B:22 C:8 D:5580

Chemistry
1 answer:
ycow [4]3 years ago
8 0

Answer: A

jk D

Explanation: because its math

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Calculate the volume of a cube with links to 2.2 in.
vlada-n [284]

Answer:

10.65

Explanation:

3 0
3 years ago
What change takes place when a liquid absorbs heat energy without increasing its temperature? A. the pressure increases B. it va
gtnhenbr [62]

B.

When water is heated, it evaporates.

4 0
4 years ago
Read 2 more answers
Which types of matter are made of atoms?
Phoenix [80]
The best and most correct answer among the choices provided by your question is the third choice or letter D.

<span>Solids, liquids, gases and plasma are all made of atoms.</span>

I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!
7 0
3 years ago
C2 H6 +02 equals CO2 + H2O what mass of water is produced from three moles of C2 H6?
yulyashka [42]

Answer:

162g

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

2C2H6 + 7O2 —> 4CO2 + 6H2O

Next, we shall determine the number of mole of water, H2O produced by the reaction of 3 moles of C2H6.

This can be obtained as follow:

From the balanced equation above,

2 moles of C2H6 reacted to produce 6 moles of H2O.

Therefore, 3 moles of C2H6 will react to produce = (3 x 6)/2 = 9 moles of H2O.

Therefore, 9 moles of H2O is produced from the reaction.

Finally, we shall convert 9 moles of H2O to grams.

This can be done as shown below:

Molar mass of H2O = (2x1) + 16 = 18g/mol

Mole of H2O = 9 moles

Mass of H2O =..?

Mole = mass / molar mass

9 = mass of H2O /18

Cross multiply

Mass of H2O = 9 x 18

Mass of H2O = 162g

Therefore, 162g of H2O were produced from 3 moles of C2H6.

8 0
3 years ago
The vapor pressure of ethanol is 54.68 mm Hg at 25°C. How many grams of estrogen (estradiol), C18H24O2, a nonvolatile, nonelectr
amm1812

Answer:

30.5 g of estrogen

Explanation:

Lowering vapor pressure formula → P° - P' = P° . Xm

P° → Vapor pressure of pure solvent → 54.68 mmHg

P' → Vapor pressure of solution → 53.46 mmHg

54.68 mmHg - 53.46 mmHg = 54.68 mmHg . Xm

0.0223 = Xm → This is the mole fraction for solute

Moles of solute / Total moles

Total moles = Moles of solute + Moles of solvent

Let's determine the moles of solvent → 228 g / 46.07 g/mol = 4.95 moles

Let's determine the moles of solute

Moles of solute / Moles of solute + 4.95 = 0.0223

Moles of solute = 0.0223 . Moles of solute + 0.110

0.9777 moles of solute = 0.110

Moles of solute = 0.110 / 0.9777 → 0.112

Now we can convert the moles to mass to finish the excersise:

0.112 mol . 272.4 g/mol = 30.5 g

3 0
3 years ago
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