Answer
531s
Explanation
Pt4+ + 4e- ---------> Pt
To deposite 1mole of Pt 4moles of electrons requirex
Initial moles of Pt4+= ( 0.025mol/1.00L) × 0.20L = 0.005mol
99% of 0.004mol = ( 0.005mol/100)× 99= 0.00495mol
moles of electrons required to deposite 0.00495moles of Pt = 4× 0.00495mol = 0.01980mol
charge of 0.01980moles of electrons = 96485C/mol ×0.01980mol = 1910.4C
1A = 1C/s
3.60A = 3.60C/s
time required = 1910.4C/3.60C/s = 531s
A solution containing Pt44 is electrolyzed with a current of 3.60 A. How long will it...
How long would it take to electrodeposit all the Cu2+ in 0.350 L of 0.240 M CuSO4 solution with an applied potential difference of 0.230 V and a current of 3.60 amperes? Enter your answer in minutes.
A Cr3+(aq) solution is electrolyzed, using a current of 6.90 A. 1. What mass of Cr(s) is plated out after 1.60 days? 2. What amperage is required to plate out 0.220 mol Cr from a Cr3+ solution in a period of 8.90 h?
Question 10 10 pts How long would It take for 6.50 g of solid copper to plate out of a solution of CuSO4(aq) being electrolyzed by a constant current of 10.0 A? 32.9 min 8.22 min 164 min 50.6min 25.3 min
A-D A. How many miles of Cu2+ is present in the solution? B. How many miles of electrons are needed to plate all the Cu2+? C. Calculate the coulombs of charge, q required to plate all Cu2+? D. How many hours will it take to plate out all the Cu2+? B. Electrodeposition A solution of 200.0 mL of a o015 M cu r solution was electrolyzed using a current, i, of 0.200 amp? The half reaction is shown below: 2...
A 1L solution containing 0.1M NiCl2(aq) and 0.2M CuBr2(aq) is subjected to electrolysis. How much time would it take to selectively plate out one of the cations at a current of 5A?
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
Which one is the metal? QUESTION 7 When a solution containing M(NO3)3 of an unknown metal M is electrolyzed, it takes 74.1 s for a current of 2.00 A to to plate out 0.0805 g of the metal. The metal A. Sm B. Cr OC. V D.Bi E. Gd Sqve All Answers to save all answers.
An unknown metal (M) is electrolyzed. Running a current of 1.50 A for 60.Os plated out 0.0496 g of the metal from a solution containing M(NO3)2. What is the metal? Faraday constant = 96, 485 C/mol O Zn O Ni Co Cu Sn O Pd
An acidic solution containing copper ions is electrolyzed, producing gaseous oxygen (from water) at the anode and copper at the cathode. For every 14.2 g of oxygen generated, 113 g of copper plates out. What is the oxidation state of the copper in the solution?
An acidic solution containing rhodium ions is electrolyzed, producing gaseous oxygen (from water) at the anode and rhodium at the cathode. For every 17.1 g of oxygen generated, 73.3 g of rhodium plates out. What is the oxidation state of the rhodium in the solution?