OU Molecular Mass and Molar Mass Discussion

Use your own words and use at least 2 scholarly sources cited.

Question #1 – Molecular Mass and Molar Mass

(NH4)2CO3

For the following chemical compounds compute the molecular mass (adding the atomic mass of each element, value that you find in the periodic table of elements, multiplied by the number of atoms in the molecules – unit will be atomic mass unit) and the molar mass (same mass as molecular mass but in grams)

Reply to discussion post:

Follow-up topics:

If a peer made a mistake in the initial post reply to your peer and walk us through how to correct the mistake, showing all work.

Reply to one of peers initial posts and use the dilution equation to prepare a more dilute solution. You may choose the final dilution that you are aiming for, just be sure that your chosen concentration is less than the initial concentration in your peers posting. Show all work and walk us through each step of how you would prepare this solution from your peer’s solution in a lab setting.

Find an example of an important chemical reaction used in industry or clinical setting and do each the following. Note, you cannot choose the same reaction as a peer.

Explain the significance of the reaction you chose. 

State the reaction without the use of any coefficients so that a peer can balance the chemical reaction your discussed

Balance a peers chemical equation by following the steps below:

Determine the number of atoms for each compounds in the reactants.

Determine the number of atoms for each compounds in the products.

Balance the chemical reaction, showing all work.

Peer Discussion Post:

Hello Class,

I chose Option 2- 1.25) C6H10O4

Question #1 – Molecular Mass and Molar Mass

C6H10O4- molecule contains:

• six carbon, ten hydrogen, and four oxygen atoms
• Element: Hydrogen
  Symbol: H
  Atomic Mass: 1.00794
  # of Atoms: 10
  Mass Percent: 6.897%
• Element: Carbon
  Symbol: C
  Atomic Mass: 12.0107
  # of Atoms: 6
  Mass Percent: 49.311%

Element: Oxygen
Symbol: O
Atomic Mass: 15.9994
# of Atoms: 4
Mass Percent: 43.792%

• molecular mass 72.0642 g/mol + 10.0794 g/mol + 63.9976 g/mol = 146.1412 g/mol
• molar mass of 146.14 g/mol
• Option #2- 2.25) HgO->Hg + O2.

Question #2 Balancing Chemical Equations

• To balance a chemical equation:
• Every element must have the same number of atoms on each side of the equation (law of conservation of mass).
• Balancing the equation can be done only by adjusting the coefficients.

Hg is a balanced element because there is the same number of atoms of Hg in each side of the equation.

Hg is a balanced element.

O is not a balanced element. To balance O, multiply HgO from the left side by 2.

2HgO?Hg+O2

Hg is not a balanced element. To balance Hg, multiply Hg from the right side by 2.

2HgO?2Hg+O2

O is a balanced element because there is the same number of atoms of O on each side of the equation.

O is a balanced element

All elements have the same number of atoms in each side of the equation, which means that the law of conservation of mass is satisfied, and the chemical equation is balanced.

2HgO?2Hg+O2