Questions LLC
Login
or
Sign Up
Ask a New Question
Science
Chemistry
An electroplating cell operates for 35 min with a current of 1,9 A. Calculate the amount, in mols, of electrons transferred.
1 answer
amperes x seconds = coulombs
96,485 coulombs = 1 mol electrons
You can
ask a new question
or
answer this question
.
Related Questions
In the gas-phase reaction given below, the [I2] changes from 0.400 M at 0.00 min to 0.200 M at 3.00 min. I2 + Cl2 --> 2 ICl
A cell of emf 2v and internal resistance of 1ohms passes a current through an external load of 9ohms.calculate the potential
An X-ray tube used for cancer therapy operates at 4.04 MV with a beam current of 23.4 mA striking a metal target. Calculate the
A step down transformer operates a 2400 volt lines and supplies a current of 60A.The turn ratio of the transformer is
Which of the following processes uses a galvanic cell?
A. Electroplating silver metal onto a teapot B. Purification of metals
The following electrochemical cell can be used to calculate the formation constant Kf for a metal and EDTA. The cell has a
A man swim at a speed of 50m/min, swims 100m against the current and 100m with the current. if the time difference between the
Calculate the average disappearance of A between t=0 min and t=10 min in units of M/s.
0 min there are .065 moles of A 10 min
How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through
A voltaic cell utilizes the following reaction and operates at 298K
3Ce{4+}(aq)+Cr(s)--->3Ce{3+}(aq)+Cr{3+}(aq) {}=Charge What is