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Novay_Z [31]
2 years ago
5

What is the molar mass of Al2(SO4)3

Chemistry
2 answers:
Goshia [24]2 years ago
8 0
Molar mass= <span>342.15 g/mol</span>
andrey2020 [161]2 years ago
4 0

Answer:

341.97 g/mol

Explanation:

Let us first write down the relative atomic masses of all the elements involved. (Please not that these will differ from periodic table to periodic table. Familiarize yourself with the data sheet in your institution)

Al - 26.892

S - 32.066

O - 15.999

From the formula we can see that we

Two aluminium atoms = 26.892*2 = 53.784

Three sulphur atoms = 32.066*3 = 96.198

Twelve oxygen atoms  = 191.988

Add them all up = 341.97

So the molar mass is 341.97 g/mol. The units have to assigned because this is the molar mass. Relative molecular mass has not units

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Why did Bromophenal solutions change from yellow to blue(what chemical reaction happended)?
MaRussiya [10]
Phenolphthalein Phenolphthalein is a universal indicator, which means it changes color to show the pH of certain solutions. Phenolphthalein stays colorless in acidic solutions and turns pink in alkaline solutions. Sodium hydroxide is a base, so when you add phenolphthalein, the solution turns pink. Other indicators commonly used in the laboratory are litmus and methyl orange. A Litmus indicator solution goes red in acidic solutions, blue in alkaline solutions and purple in neutral solutions. Methyl orange turns red in acidic solutions and yellow in neutral or alkaline solutions.
6 0
3 years ago
A 6.175 gram sample of an organic compound containing only C, H, and O is analyzed by combustion analysis and 13.30 g CO2 and 5.
Bingel [31]

Answer:

Empirical and molecular formulas are the same, C₅H₁₀O₂.

Explanation:

Hello!

In this case, when determining the empirical and molecular formulas of organic compounds via combustion analysis, we first need to compute the moles of carbon and hydrogen via the yielded mass of carbon dioxide and water:

n_C=13.30gCO_2*\frac{1molCO_2}{44.01gCO_2}*\frac{1molC}{1molCO_2}=0.30molC\\\\n_H=5.447gH_2O*\frac{1molH_2O}{18.02gH_2O}*\frac{2molH}{1molH_2O}=0.60molH

Next, we need to compute the mass of oxygen by subtracting the mass of carbon and hydrogen to the mass of the sample of the compound:

m_O =6.175g-0.3molC*12.01gC/molC-0.6molH*1.01gH/molH =1.966gO

And consequently the moles:

n_O=0.12molO

Now, we need to divide the moles of each atom by the fewest moles, it in this case, those of oxygen to obtain the subscripts in the empirical formula:

C=\frac{0.30}{0.12} =2.5\\\\H=\frac{0.60}{0.12} =5\\\\O=\frac{0.12}{0.12} =1

Thus, the empirical formula, taken the nearest whole number is:

C_5H_{10}O_2

Now, if we divide the molar mass of the molecular formula (102.1 g/mol) by that of the empirical formula (102.1 g/mol) we infer they are both the same.

Best regards!

6 0
2 years ago
Express the frequency in inverse seconds of n=4 to n=3
HACTEHA [7]

Answer:

1.60×10¹⁴ s⁻¹

Explanation:

When an electron jumps from one energy level to a lower energy level some energy is released in the form of a photon.

4 0
3 years ago
If pea plants with the genotypes RR and rr cross, what genotype will their offspring all have?
Aliun [14]
I think it’ll be Rr
6 0
2 years ago
Read 2 more answers
.an open flask contains 0.200 mol of air. atmospheric pressure is 745 mmhg and room temperature is 68˚f. how many moles are pres
aleksklad [387]

<u>0.219 moles </u><u>moles are present in the flask when the </u><u>pressure </u><u>is 1.10 atm and the temperature is 33˚c.</u>

What is ideal gas constant ?

  • The ideal gas constant is calculated to be 8.314J/K⋅ mol when the pressure is in kPa.
  • The ideal gas law is a single equation which relates the pressure, volume, temperature, and number of moles of an ideal gas.
  • The combined gas law relates pressure, volume, and temperature of a gas.

We simple use this formula-

The basic formula is PV = nRT where. P = Pressure in atmospheres (atm) V = Volume in Liters (L) n =  of moles (mol) R = the Ideal Gas Law Constant.

68F = 298.15K

V = nRT/P = 0.2 * 0.08206 * 298.15K / (745/760) = 4.992Liters

n = PV/RT = 1.1atm*4.992L/(0.08206Latm/molK * 306K)

n = 0.219 moles

Therefore, 0.219 moles moles are present in the flask when the pressure is 1.10 atm and the temperature is 33˚c.

Learn more about ideal gas constant

brainly.com/question/3961783

#SPJ4

4 0
1 year ago
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