Chemistry, 16.09.2021 20:50 diametriagay
A 2.005 sample of xCuSO4 yH2O was heated to drive off water from the hydrated salt. The anhydrous salt weighed 1.283 grams.
a. What is the mass of water lost.
b. How many moles of water were lost.
c. How many moles of anhydrous salt remain.
d. What is the empirical formula for the hydrate (Ration x:y).
Answers: 3
Chemistry, 22.06.2019 14:30
Consider the reduction reactions and their equilibrium constants. cu+(aq)+e−↽−−⇀cu(s)pb2+(aq)+2e−↽−−⇀pb(s)fe3+(aq)+3e−↽−−⇀fe(=6.2×108=4.0×10−5=9.3×10−3 cu + ( aq ) + e − ↽ − − ⇀ cu ( s ) k =6.2× 10 8 pb 2 + ( aq ) +2 e − ↽ − − ⇀ pb ( s ) k =4.0× 10 − 5 fe 3 + ( aq ) +3 e − ↽ − − ⇀ fe ( s ) k =9.3× 10 − 3 arrange these ions from strongest to weakest oxidizing agent.
Answers: 3
Chemistry, 22.06.2019 19:50
A2.5% (by mass) solution concentration signifies that there is a 2.5 % (by mass) solution concentration signifies that there is blank of solute in every 100 g of solution. of solute in every 100 g of solution
Answers: 3
A 2.005 sample of xCuSO4 yH2O was heated to drive off water from the hydrated salt. The anhydrous sa...
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