A solution of a copper (II) salt is electrolyzed with a 2.00 ampere current for 10 minutes. What mass of metallic copper is obtained?
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A solution of a copper (II) salt is electrolyzed with a 2.00 ampere current for 10...
A 1M aqueous solution of copper(II) nitrate is electrolyzed. What are the predicted products at the anode and cathode? NO2 gas at the anode; copper metal at the cathode NO2 gas at the anode; H2 gas at the cathode N2 gas at the anode; copper metal at the cathode O2 gas at the anode; copper metal at the cathode O2 gas at the anode; H2 gas at the cathode
A 1M aqueous solution of copper(II) nitrate is electrolyzed. What are the predicted products at the anode and cathode? NO2 gas at the anode; copper metal at the cathode NO2 gas at the anode; H2 gas at the cathode N2 gas at the anode; copper metal at the cathode O2 gas at the anode; copper metal at the cathode O2 gas at the anode; H2 gas at the cathode
Be sure to answer all parts. When an aqueous solution containing gold (III) salt is electrolyzed, metallic gold is deposited at the cathode, and oxygen gas is generated at the anode. (a) If 6.05 g of Au is deposited at the cathode, calculate the volume of 02 generated at 23°C and 752 mmHg. (b) What is the current used if the electrolytic process took 4.30 h?
Be sure to answer all parts. When an aqueous solution containing gold (III) salt is electrolyzed, metallic gold is deposited at the cathode, and oxygen gas is generated at the anode. (a) If 7.49 g of Au is deposited at the cathode, calculate the volume of O2 generated at 23°C and 740 mmHg. L (b) What is the current used if the electrolytic process took 6.90 h? A
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Page 2 8. Indicate what reaction occurs at each electrode during electrolysis (i) Cul2(aq) (ii) MgF2(aq) (ii) CdCl21) (molten salt) 9. A current of 2.50 A is passed through a solution of Cu(NO3)2 for 2.00 hr. What mass of copper is deposited at the cathode?
Page 2 8. Indicate what reaction occurs at each electrode during electrolysis (i) Cul2(aq) (ii) MgF2(aq) (ii) CdCl21) (molten salt) 9. A current of 2.50 A is passed...
you need to make 2.00 L of 0.05 M copper (II) nitrate solution. How many grams of copper (II) nitrate will you require?
CuSO4• 5H20 -------> Custy + D u 2) What is the color for anhydrous salt of copper (II) sulfate (CuSO4)? What is the color for ionic hydrate compound of copper (II) sulfate pentahydrate (CuSO4.5H2O)? 3) How would you test a colorless crystalline compound to determine whether it is a hydrate or not? 4) How many grams of CuSO4.5H20 are needed to prepare 50.0 mL of a 1.00 M CuSO4 solution? 5) Suppose you used the Procedure in this experiment to...
How many grams of copper will be plated out by a current of 2.3 A applied for 5.0 minutes to a 0.50 M solution of copper (II) sulfate? How many grams of copper will be plated out by a current of 2.3 A applied for 5.0 minutes to a 0.50 M solution of copper (II) sulfate? 1.8 × 10-2 0.23 0.45 0.019 3.6 × 10-2
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?
A tube containing 8.00 mL of 0.250 M copper (II) sulfate contains 2.00 x 10^-3 mole of copper (II) sulfate. how many grams of solid copper (II) sulfate would this be equivalent to? using dimensional analysis