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MA_775_DIABLO [31]
3 years ago
12

What is the empirical formula for C 57.66

Chemistry
1 answer:
ELEN [110]3 years ago
4 0

C5H12O2 (2-ISOPROPOXYETHANOL)

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anyanavicka [17]
It does<span>, however, change the </span>mass<span> of the nucleus. </span>Adding<span> or removing </span>neutrons<span>from the nucleus are how isotopes are created. Protons carry a positive electrical charge and they alone determine the charge of the nucleus.</span>
7 0
3 years ago
Dihydrogen dioxide decomposes into water and oxygen gas. Calculate the amounts requested if 1.34 moles of dihydrogen dioxide rea
a_sh-v [17]

Answers:

<em><u>a. Moles of oxygen formed:</u></em><u> 0.670 mol</u>

<em><u>b. Moles of water formed:</u></em><u> 1.34 mol</u>

<em><u>c. Mass of water formed:</u></em><u> 24.1 g</u>

<em><u>d. Mass of oxygen formed:</u></em><u> 21.4 g</u>

<u></u>

Explanation:

Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.

The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:

2H_2O_2(l)\rightarrow 2H_2O(l)+O_2(g)

The mole ratios derived from that balanced chemical equation are:

  • 2 mol H₂O₂ : 2 mol H₂O : 1 mol O₂

<em><u>a. Moles of oxygen formed</u></em>

  • Set the proportion using the theoretical mole ratio of H₂O₂ to O₂ and the amount of moles of dyhydrogen dioxide that react:

2\text{ mol }H_2O_2/1\text{ mol }O_2=1.34\text{ mol }H_2O_2/x

When you solve for x, you get:

  • x = 1.34 mol H₂O₂ × 1 mol O₂ / 2 mol H₂O₂ = 0.670 mol O₂

<u />

<em><u>b. Moles of water formed</u></em>

  • Set the proportion using the theoretical mole ratio of H₂O₂ to H₂O and the amount of moles of dyhydrogen dioxide that react:

2\text{ mol }H_2O_2/2\text{ mol }H_2O=1.34\text{ mol }H_2O_2/x

When you solve for x, you get:

  • x = 1.34 mol H₂O₂ × 2 mol H₂O / 2 mol H₂O₂ = 1.34 mol H₂O

<em><u>c. Mass of water formed</u></em>

Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:

  • Molar mass of water = 18.015 g/mol

  • Number of moles = mass in grams / molar mass

       ⇒ mass in grams = number of moles × molar mass

       ⇒ mass in grams = 1.34 mol × 18.015 g/mol = 24.1 g

<em><u>d. Mass of oxygen formed</u></em>

Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.

  • Molar mass of O₂ = 32.00 g/mol
  • mass = molar mass × number of moles
  • mass = 32.00 g/mol × 0.670 mol = 21.4 g.
5 0
3 years ago
How many moles of sulfur atoms are in 9.9 moles of Ag2S
GarryVolchara [31]

Answer:

9.9 moles of Ag₂S contain 9.9 moles of sulfur.

Explanation:

Given data:

Number of moles of Ag₂S = 9.9 mol

Number of moles of Sulfur = ?

Solution:

One mole of Ag₂S having 1 mole of sulfur.

In 9.9 moles:

9.9 moles × 1 = 9.9 moles

So 9.9 moles of Ag₂S contain 9.9 moles of sulfur.

6 0
3 years ago
Calculate the ratio of effusion rates for ar and kr.
Natali [406]
Atomic mass Kr = 83.8 g/mole
Atomic mass Ar = 39.948 g/mole

So the ratio of the effusion rates = SQRT(83.8/39.948) = 1.45. Argon moves 45% faster than krypton!

Hope that helped!
4 0
3 years ago
Write an equation to solve for the mass of oxygen. mass of ? = mass of ? = mass of ?
Alina [70]

Answer:

Explanation:

we know that number of moles=mass(in grams)/molar mass

for the mass of oxygen the equation becomes

mass=number of moles*molar mass

8 0
3 years ago
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