All categories

2 months ago

15 g of gold and 25 g of silver are mixed to form a single-phase ideal solid solution.

1 answer:

8 0

1. The total moles of the solution is 0.3079193 mol. 2. The mole fraction for gold is 0.2473212, and for silver, it is 0.7526787. 3. The molar entropy of mixing for gold is 2.87285 j/K, while for silver, it is 1.77804 j/K. 4. The total entropy of mixing sums to 4.65089 j/K. 5. Molar free energy amounts to -2325.445 kJ. 6. Chemical potential for silver is -1750.31129 j/mol and for gold, it is -575.13185 j/mol. To elaborate: (1) The molar mass of silver stands at 107.8682 g/mol, and gold's at 196.96657 g/mol. Hence, calculating moles leads to mass/molar mass for silver: 25 g/107.8682 g/mol = 0.2317643 mol and for gold: 15 g/196.96657 g/mol = 0.076155 mol, resulting in a total of 0.30791193 mol. (2) For the mole fractions, silver's fraction is 0.2317643/0.3079193 = 0.7526787, and for gold, it's 0.076155/0.3079193 = 0.2473212. (3) To find molar entropy mixing ∆Sm, we use the formula ∆Sm = -R * Xi * ln(Xi) where R = 8.3144598. For silver, substituting gives us 1.77804 j/K, while for gold, we get 2.87285 j/K. (4) Overall entropy of mixing totals 4.65089 j/K thus calculated. (5) The Gibbs free energy at 500 °C can be derived through G = H - TS, accounting to H = 0 (as T is 500 + 273 = 773 K and S is 4.65089), resulting in G equating to -3595.138 kJ. (6) The chemical potentials calculated derive from multiplying the Gibbs free energy by their mole fractions.

You might be interested in

How many atoms of Mg are present in 97.22 grams of Mg?

VMariaS [2998]

Answer: The correct choice is (b).

Explanation:

We have the mass of Magnesium at 97.22 g, and the molar mass of Magnesium is 24.305 g/mol.

Therefore, the calculation for the number of moles is as follows.

Number of moles = $\frac{mass given in grams}{Molar mass}$

= $\frac{97.22 g}{24.305 g/mol}$

= 4 mol

Additionally, it is known that one mole contains $6.023 \times 10^{23}$ atoms/mol. Thus, we calculate the total number of atoms in 4 moles as follows.

$4 mol \times 6.023 \times 10^{23} atoms/mol$

= $24.08 \times 10^{23}$ atoms

or, = $2.408 \times 10^{23}$ atoms

Hence, we conclude that in 97.22 grams of Magnesium, there are $2.408 \times 10^{23}$ atoms.

7 0

3 months ago

Which statement explains why sulfur is classified as a Group 16 element?

Tems11 [2777]

Answer: The correct option is (1).

Explanation:

Group 16 is the third-from-last column in the periodic table and is known as the oxygen family.

Members of this group include oxygen, sulfur, selenium, tellurium, and polonium.

Elements in Group 16 have 6 valence electrons in their outermost shell.

The electronic configuration of sulfur is $1s^22s^22p^63s^23p^4$ .

Because sulfur belongs to Group 16, it has 6 valence electrons.

3 0

2 months ago

Read 2 more answers

If the following elements were to form ions, they would attain the same number of electrons as which noble gas? As , Be , O , S

Alekssandra [3086]

Answer;

As and Sr ------- [Kr]

Be ------------- [He]

O and Mg ------- [Ne]

S and Ca ------- [Ar]

Explanation

The Be+ ion has 2 electrons, matching He. The Mg2+ and O2− ions possess 10 electrons each, like Ne.
S2− and Ca2+ ions each have 18 electrons, the same as Ar. The As3− and Sr+ ions hold 36 electrons, paralleling Kr.
Elements gain or lose electrons to reach a stable electron configuration akin to that of noble gases.
When atoms lose electrons, they form positive ions (cations), and when they gain electrons, they form negative ions (anions).

4 0

4 months ago

Read 2 more answers