Question

What’s the molar mass for zinc nitrate?

Answer 1

Zn (No3)2

zinc is a transition metal, thats why there is a 2 outside the bracket, its because most transitions metals oxidation number is 2 or 3

Molar mass

Zn = 65

N = 14 (2) = 28

O = 16 (3) (2) = 96

so 65+28+96 = 189g

Answer 2

The molar mass of zinc nitrate, Zn(NO3)2, is calculated by summing the atomic masses of one zinc atom (65.38 g/mol) and two nitrate ions (28.02 g/mol for nitrogen and 96.00 g/mol for oxygen), resulting in a molar mass of 189.40 g/mol.

Step-by-step explanation:

The molar mass of zinc nitrate, Zn(NO3)2, is calculated by adding the atomic masses of zinc (Zn) and two nitrate ions (NO3). Using the atomic masses from the periodic table, we have:

• 1 Zn = 65.38 g/mol
• 2 N (from NO3, 2 moles) = 14.01 g/mol × 2 = 28.02 g/mol
• 6 O (from 2 NO3, or 6 moles) = 16.00 g/mol × 6 = 96.00 g/mol

Adding these together, the molar mass of Zn(NO3)2 is:

65.38 g/mol + 28.02 g/mol + 96.00 g/mol = 189.40 g/mol.

The molar mass is crucial for mass-mass calculations to determine theoretical yield or percent yield in a reaction involving zinc nitrate. For instance, if the actual yield from a reaction is known, the percent yield can be calculated by dividing the actual yield by the theoretical yield and multiplying by 100.