You perform an electrochemical reaction in which 0.600 mol of Cu are reduced to solid Cu. How many coulombs of charge are transferred?How many electrons are in this amount of charge?

Explanation:

Step 1: Write the reaction for the electrochemical reduction of copper.

Cu²⁺(aq) + 2 e⁻ → Cu(s)

Step 2: Calculate the number of electrons required in the reduction of 0.600 moles of Cu²⁺

We will use the following relationships:

Step 3: Calculate the Coulombs corresponding to

We will use the following relationships:

h let me think

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm