Assume that silver and gold form ideal, random mixtures. Calculate the mass of pure Ag needed to cause an entropy increase of 20 J/K when mixed with 100g of pure Au

Explanation:

Hello!

In this case, since the definition of entropy in a random mixture is:

For this silver-gold mixture we write:

By knowing the moles of gold:

It is possible to write the aforementioned formula in terms of the variable representing the moles of silver:

Which can be solved via Newton-Raphson or a solver software, in this case, I will provide you the

So the mass is:

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explanation:

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).