In an electroplating process, copper (ionic charge +2e, atomic weight 63.6 g/mol) is deposited using a current of 10.0 a. what mass of copper is deposited in 10.0 minutes? avogadro's number is 6.022 × 1023 molecules/mol and e = 1.60 × 10-19 c.

Answer : The mass of copper deposit is, 1.98 grams

Explanation :

First we have to calculate the charge.

Formula used :

where,

Q = charge = ?

I = current = 10 A

t = time = 10 min = 600 sec      (1 min = 60 sec)

Now put all the given values in this formula, we get

Now we have to calculate the number of atoms deposited.

As, 1 atom require charge to deposited =  

Number of atoms deposited = atoms

Now we have to calculate the number of moles deposited.

Number of moles deposited = moles

Now we have to calculate the mass of copper deposited.

1 mole of Copper has mass = 63.5 g  

Mass of Copper Deposited =

Therefore, the mass of copper deposit is, 1.98 grams

a:

by the combination of an unlimited number of elements

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer