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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substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.