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Answer:
The electrochemical equivalent of copper, Cu, is 3.29015544 × 10⁻⁷ g/C
Explanation:
The given parameters are;
The element for which the electrochemical equivalent is sought = Copper
The atomic mass of copper = 63.5
The electrochemical equivalent, 'Z', of an element or a substance is the mass, 'm', of the element or substance deposited by one coulomb of electricity, which is equivalent to a 1 ampere current flowing for a period of 1 second
Mathematically, we have;
m = Z·I·t = Z·Q
We have;
Cu²⁺ (aq) + 2·e⁻ → Cu
Therefore, one mole of Cu, is deposited by 2 moles of electrons
The charge carried one mole of electrons = 1 Faraday = 96500 C
∴ The charge carried two moles of electrons, Q = 2 × 96500 C = 193,000 C
Given that the mass of an atom of Cu = 63.5 a.m.u., the mass of one mole of Cu, m = 63.5 g
∴ Z = 3.29015544 × 10⁻⁴ g/C = 3.29015544 × 10⁻⁷ g/C
The electrochemical equivalent of copper, Cu, is Z = 3.29015544 × 10⁻⁷ g/C
Answer:
root mean square velocity of nitrogen at 25°c is 515 m/s
correct option is b) 515 m/s
Explanation:
given data
temperature = 25°c = 25 + 273 = 298 K
to find out
root mean square velocity of nitrogen molecules
solution
we know that root mean square velocity of gas is Vrms = .......................1
mass of gas = M
universal gas constant = R
temperature = T
and we know mass of nitrogen = 28 g = 28 × kg
Vrms =
Vrms =
Vrms = 515.22 m/s
root mean square velocity of nitrogen at 25°c is 515 m/s
correct option is b) 515 m/s