. Suppose that you have an unlimited supply of copper II chloride to react with iron....
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. Suppose that you have an unlimited supply of copper II
chloride to react with iron....
Hydroxylammonium chloride reacts with iron(II) chloride, FeCl, in solution to produce ironIl) chloride, HCL iron(II) chloride,...
Hydroxylammonium chloride reacts with iron(II) chloride, FeCl, in solution to produce ironIl) chloride, HCL iron(II) chloride, HCl H2O, and a compound of nitrogen. It was found that 2.00g of iron(II) chloride reacted in this way with 31.0 mL of 0.200M hydroxylammonium chloride. Suggest a possible formula for the compound of nitrogen so produced. This should be a known nitrogen compound.
Let's say you have 25mL of a 3.25M copper (II) chlorate solution a) what is the...
Let's say you have 25mL of a 3.25M copper (II) chlorate solution a) what is the chemical formula of copper (II) chlorate? b) how many moles of copper (II) chlorate would be in the solution? c) How many moles of the copper (II) ion would be in the solution? d) How many of the chlorate ion would be in the solution? e) How many molecules of copper (II) chlorate would be in the solution? f) How many atoms of oxygen...
1.00 g of Mg metal was added to a solution of Copper (II) chloride resulting in...
1.00 g of Mg metal was added to a solution of Copper (II) chloride resulting in the precipitation of metallic copper. The solution remained blue after all the Mg had reacted: a. write a balanced equation. b. How many moles of Mg was added to the solution? c. How many moles of Copper was precipitated? d. How many grams of Copper was precipitated?
How many moles of iron would have been used up if 48.0 g of copper were...
How many moles of iron would have been used up if 48.0 g of copper were to be produced?
Practice 1. An aluminum wire is placed in 60.0 mL of an unknown copper(II) chloride dihydrate solution. The copper(II)...
Practice 1. An aluminum wire is placed in 60.0 mL of an unknown copper(II) chloride dihydrate solution. The copper(II) and aluminum react in the redox reaction below, producing solid copper: 3 Cu (aq) 2 Al(s) -3 Cus) 2 Al (aq) The solid copper was filtered using a Büchner funnel, and then was dried one time and weighed to be 0.256 g. It was dried a second time and weighed to be 0.235 g. It was dried a third time and...
How many moles of ammonia would be required to react exactly with 0.482 moles of copper(II)...
How many moles of ammonia would be required to react exactly with 0.482 moles of copper(II) oxide in the following chemical reaction? 2 NH₃ (g) + 3 CuO (s) → 3 Cu (s) + N₂ (g) + 3H₂O (g)
please answer question correctly and show your work! Suppose 2.26 g of Iron(II) chloride is dissolved...
please answer question correctly and show your work!
Suppose 2.26 g of Iron(II) chloride is dissolved in 250. ml of a 38.0 m M aqueous solution of silver nitrate. Calculate the final molarity of iron(II) cation in the solution. You can assume the volume of the solution doesn't change when the iron(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits. M
16 Cts with aqueous copper(II) chloride accord- 101. Zinc metal reacts with aqueous copper(1) ing to...
16 Cts with aqueous copper(II) chloride accord- 101. Zinc metal reacts with aqueous copper(1) ing to this equation: Zn (s) + CuCl2 (aq) → ZnCl2 (aq) + Cu (s) In this reaction, what mass of copper metal can be pro- duced from the reaction of 500 mL of 1.20-M aq. cu 2 with excess zinc? 10 103. The concentration of bromide ion may be determined by gravimetric analysis, using this reaction: Ag+ (aq) + Br (aq) → AgBr (s) A...
Copper Nitrate and Zinc - Moles of Copper Preciptate
If you react 1 mole of zinc with a copper (II) nitrate solution, how many moles of copper preciptate do you have?I assume this is "1", but I'm confused about if I need to know the number of moles of the copper (II) nitrate solution or not?
A student determines the iron(II) content of a solution by first precipitating it as iron(II) hydroxide,...
A student determines the iron(II) content of a solution by first precipitating it as iron(II) hydroxide, and then decomposing the hydroxide to iron(II)oxide by heating. How many grams of iron(II) oxide should the student obtain if his solution contains 31.0 mL of 0.590 M iron(II) nitrate? g ed Submit Answer Retry Entire Group 2 more group attempts remaining
Hydroxylammonium chloride reacts with iron(II) chloride, FeCl, in solution to produce ironIl) chloride, HCL iron(II) chloride, HCl H2O, and a compound of nitrogen. It was found that 2.00g of iron(II) chloride reacted in this way with 31.0 mL of 0.200M hydroxylammonium chloride. Suggest a possible formula for the compound of nitrogen so produced. This should be a known nitrogen compound.
Practice 1. An aluminum wire is placed in 60.0 mL of an unknown copper(II) chloride dihydrate solution. The copper(II) and aluminum react in the redox reaction below, producing solid copper: 3 Cu (aq) 2 Al(s) -3 Cus) 2 Al (aq) The solid copper was filtered using a Büchner funnel, and then was dried one time and weighed to be 0.256 g. It was dried a second time and weighed to be 0.235 g. It was dried a third time and...
please answer question correctly and show your work!
Suppose 2.26 g of Iron(II) chloride is dissolved in 250. ml of a 38.0 m M aqueous solution of silver nitrate. Calculate the final molarity of iron(II) cation in the solution. You can assume the volume of the solution doesn't change when the iron(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits. M
16 Cts with aqueous copper(II) chloride accord- 101. Zinc metal reacts with aqueous copper(1) ing to this equation: Zn (s) + CuCl2 (aq) → ZnCl2 (aq) + Cu (s) In this reaction, what mass of copper metal can be pro- duced from the reaction of 500 mL of 1.20-M aq. cu 2 with excess zinc? 10 103. The concentration of bromide ion may be determined by gravimetric analysis, using this reaction: Ag+ (aq) + Br (aq) → AgBr (s) A...
A student determines the iron(II) content of a solution by first precipitating it as iron(II) hydroxide, and then decomposing the hydroxide to iron(II)oxide by heating. How many grams of iron(II) oxide should the student obtain if his solution contains 31.0 mL of 0.590 M iron(II) nitrate? g ed Submit Answer Retry Entire Group 2 more group attempts remaining
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