CHEMISTRY HIGH SCHOOL

If you use 19 mL of 0.100 M KMnO4, how many moles have you used? The answer has to be in four decimal places (do not forget the leading zero). No scientific notation.How much 5.0 M H2SO4 needs to be used to make 152 mL of 1.0 M? Round answer to nearest whole number and omit units.

Answers

Answer 1
Answer: 1)

Volume = 19 / 1000 = 0.019 L

n = M * V

n = 0.100 * 0.019

n = 0.0019 moles
__________________________

2)

 M₁ * V₁ = M₂* V₂

5.0 * V₁ = 1.0 * 152

5.0 V₁ = 152

V₁ = 152 / 5.0

V₁ = 30.4 mL
______________________________________

hope this helps!

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How many moles of atoms are in 6.00 g of 13C?

Answers

There are 0.462 moles of atoms in 6.00 g of carbon-13.

Further Explanation:

Moles, Atomic mass and Molecular mass  

  • 1 mole of a pure substance contains a mass that is equal to the relative atomic mass or molecular mass of the substance.
  • Therefore; molar mass is given as grams per mole of a substance  
  • Hence;

Molar mass = mass of a substance/ Number of moles

     g/mol = g /mole

  • Thus:

M = m/n; where M is the molar mass, m is the mass and n is the number of moles

  • From this relationship we can therefore, calculate mass by multiplying the number of moles by molar mass of a substance.
  • That is; Mass = moles x molar mass
  • To calculate number of moles;

We have; n = m/M

  • Number of moles = Mass of the substance/ Molar mass

In our case;

Mass = 6 g of Carbon-13

Molar mass = 13.0 g/mol

Since; Number of moles = Mass/ molar mass

Thus;

Moles = (6.0 g)/ (13.0 g/mol)

          = 0.462 moles  

Keywords: Moles, Molecular mass, relative atomic mass  

Learn more about:

Level: High school

Subject: Chemistry

Topic: Moles

Sub-topic: Moles, molecular mass and mass of a pure substance

Answer: 0.462 moles

Explanation: 13C indicates an isotope of carbon and its mass number is 13. It means the mass of 1 mol of 13C is 13 gram.

The question asks to calculate the number of atoms present in 6.00 grams of 13C.

To calculate the number of moles we divide the given grams by the mass of 1 mol of the element. The set could be shown easily using dimensional analysis as:

6.00gram((1mol)/(13gram))

= 0.462 moles

So, there will be 0.462 moles of atoms in 6.00 grams of 13C.

Fe2O3 + H2 --> Fe + H2OA) what mass of hydrogen gas must be consumed to produe 10.0 g of iron metal?

B) what mass of iron(lll) oxide, Fe2O3, must be consumed to prepare 2.50g of iron metal

Answers

A) 10.0g of Iron is (10.0)/(55.8)=179mmol of Iron.

One mole of dihydrogen is required to form one mole of iron, hence you'll need 0.179*1.00=0.179g of dihydrogen.

B) Likewise : 2.50g of Iron is (2.50)/(55.8)=44.8mmol of Iron, hence we'll need 44.8*(3*16+2*55.8)=7.15g of Fe2O3.

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Answers

Answer:

D. A process that breaks down large rocks into smaller pieces.

Explanation:

Physical weathering if referred to the process of rocks breaking apart without changing their chemical composition. If you look at the other answers, none of them match the description of physical weathering.

Answer:

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Answers

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Answers

Answer: Empirical formula

Empirical formula referst to the simplest whole-number ration of atoms in a molecule. A compound's molecular formula can either be the same or multiple of its empirical formula. The structural and molecular formulas are also part of the compound formulas
Hi there! The simplest whole-number ratio of the atoms in a molecule of formula is called the Empirical formula.

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