Nickle hyrdoxide reacting with hydrazine?

Question

10 grams of nickel (II) hydroxide is mixed with 1.0< aqueous solution of hydrazine (density = 1.05g/ml).

Using the density of the given solution, determine the grams of hyrazine solution required.

Based on the starting weight of nickel (II) hydroxide, how much Nickel should have been produced?

PLEASE SHOW ME HOW YOU FOUND YOUR ANSWERS!!

I got the balanced equation to be:::

2Ni(OH)2 + N2H4 ---> 2Ni + N2 + 4H2O

Answer 1

The question is a bit unclear.

If &quot;mixed with 1.0&lt; aqueous solution&quot; means 1.0 molar solution, a calculation can be made.

The molar mass of Ni(OH)2 is 58.7 + 32 + 2 = 92.7 g/mol. Your 10g sample will have 10/92.7 mol NiOH2, and require the same amount of mols hydrazine. Since you have a 1.0 mol/l solution, each mol will require 1l of hydrazin solution. With density 1.05 g/ml, or 1.05 kg/l, multiply that number by 1050 to get the grams.