Question

1- Write the equilibrium constant expression for this reaction:

NH3(aq)+H+(aq)→NH+4(aq)

2- A chemist prepares a solution of zinc oxalate ZnC2O4 by measuring out 1.6mg of zinc oxalate into a 500.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L  of the chemist's zinc oxalate solution. Round your answer to 2 significant digits.

3- Wine goes bad soon after opening because the ethanol CH3CH2OH  dissolved in it reacts with oxygen

O2  gas to form water and aqueous acetic acid CH3COOH, the main ingredient in vinegar. Calculate the moles of oxygen needed to produce

0.085mol  of acetic acid. Be sure your answer has a unit symbol, if necessary, and round it to 2  significant digits.

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. ol. 1 - Ca(C102), (aq) + H20(1) 0-0 18 Ar x $ ?

Answer 1

1. k : [Ne (NH3] [kt] Amount 2. 1.6 x 10 gm 1.6. mg 500 ml 0.5 e म 155-4 gmor of zinc oxalate Volume solution Molar weight of zinc onatete- Molarity moles of zinc onalate Volume of solution (1) 1.6 x 103 ym = 155.4 0.5 e gmolt x = 2.059 x 10 tos mol/l 3. Ho + O2 CH₃CH₂OH + CH3coon 0.085 mol Moles of acetic acid produced to balanced equation, According

so 1 mol of O2 is needed needed to produce 1 mod. of acetic acid 0.005 moles of O. needed to produce -0.085 mol of acetic and Please Rate the Answer! keep Learning