0.222g of a divalent metal is deposited when a current of 0.4amperes is passed through a solution of it's salt for 25minutes calculate?
(I) time taken in seconds
(ii) quantity of electricity flowing
(iii) Atomic mass of the metal
time = 25 minutes x (60 sec/min) = 1500 seconds.
coulombs electricity = C = current x seconds = 0.4 amperes x 1500 sec = 600.0
96,485 coulombs will deposit (atomic mass/2) = 0.222 grams.
(atomic msss/2) x (600/96,485) = 0.222
atomic mass = 2*96,485*0.222/600 = 71.4 amu
Is this a made up problem. I don't see an atom with an atomic mass of 71.4 in the periodic table. Ge and Ga come the closest but not quite right. Ge is 72.6 and Ga is 69.7 BUT NEITHER IS DIVALENT. Gotta believe it's a made up problem.
To solve this problem, we can use the formula:
Quantity of electricity (Q) = Current (I) x Time (t)
Given:
Current (I) = 0.4 amperes
Time (t) = 25 minutes
(i) To find the time in seconds:
Since 1 minute is equal to 60 seconds, we can convert the time into seconds by multiplying it by 60.
Time in seconds = 25 minutes x 60 seconds/minute
(ii) To find the quantity of electricity flowing:
We are given the current and time, so we can plug these values into the formula to get the answer.
Quantity of electricity (Q) = 0.4 amperes x (25 minutes x 60 seconds/minute)
(iii) To find the atomic mass of the metal:
The atomic mass of the metal can be calculated by using the equation:
Atomic mass = Quantity of metal deposited / Quantity of electricity (Q)
Given:
Quantity of metal deposited = 0.222 g
Quantity of electricity (Q) = calculated in part (ii)
Atomic mass = 0.222 g / Quantity of electricity (Q)
By substituting the values for Q from part (ii) into the equation, we can find the atomic mass of the metal.
To solve this problem, we can use the formula:
Quantity of electricity (Q) = Current (I) x Time (t)
Given:
Current (I) = 0.4 amperes
Time (t) = 25 minutes = 25 x 60 = 1500 seconds
(i) To calculate the time taken in seconds, we will use the given value of time (t) which is equal to 1500 seconds.
Time taken in seconds = 1500 seconds
(ii) To calculate the quantity of electricity flowing, we will use the formula mentioned above.
Quantity of electricity (Q) = Current (I) x Time (t)
Q = 0.4 A x 1500 s
Q = 600 Coulombs
The quantity of electricity flowing is 600 Coulombs.
(iii) To calculate the atomic mass of the metal, we need to know the charge of the divalent metal ion and the Faraday's constant. The Faraday's constant is 96485 C/mol.
From the given information, we can calculate the number of moles of the metal deposited:
Number of moles = Quantity of electricity (Q) / Faraday's constant
Number of moles = 600 C / 96485 C/mol
Number of moles = 0.00622 mol
Now, we can calculate the atomic mass of the metal:
Atomic mass = Mass of the metal / Number of moles
Given that 0.222 g of the metal is deposited, we have:
Atomic mass = 0.222 g / 0.00622 mol
Atomic mass = 35.68 g/mol
The atomic mass of the metal is 35.68 g/mol.