An oxygen atom has a mass of and a glass of water has a mass of . Use this information to answer the question below. Be sure you

Answer:

Amount of salt in 1 L seawater = 34 g

Explanation:

Based on Archimedes' principle, the mass of fresh water and the mass of the cup are equal to the mass of the same volume of seawater.

The mass of freshwater can be calculated using density times volume.

1 cm³ is equivalent to 1 mL.

The mass of freshwater is 0.999 g/cm³ multiplied by 735 cm³, which results in 734.265 g.

The total mass of the freshwater and cup combined is 734.265 g plus 25 g, equating to 759.265 g.

This means the mass for an equal volume of seawater is 759.265 g.

The volume of the seawater displaced is 735 mL, which is 0.735 L (assuming the cup's volume can be disregarded).

We know that 1 liter equals 1000 cm³ or 1000 mL.

The density of seawater can be determined as mass divided by volume.

The density of seawater becomes 759.265 g divided by 0.735 L, yielding 1033.01 g/L.

Conversely, the density of freshwater in g/L is calculated as 0.999 g/(1/1000) L, equating to 999 g/L.

The mass of salt dissolved in 1 liter of seawater is calculated as 1033.01 g - 999 g, which equals 34.01 g.

Thus, the amount of salt in 1 L of seawater is 34 g.

Answer:

Can you rank the following chemical substances in order of their absolute entropies (So) from lowest (1) to highest (5) at a temperature of 298 K?

a. Al (s)

b. H2O (l)

c. HCN (g)

d. CH3COOH (l)

e. C2H6 (g)

Explanation:

Entropy quantifies the level of disorder within a system.

In solids, the entropy is significantly lower compared to liquids and gases.

The typical order of entropy is:

solids < liquids < gases

In the substances listed, liquid water notably exhibits strong intermolecular hydrogen bonding.

This results in water having comparatively lower entropy.

Next in line is acetic acid.

Among the gaseous components, ethane has higher entropy than HCN due to its weaker intermolecular interactions.

HCN involves some hydrogen bonding.

Thus, the order of entropy is:

Al(s) < CH3COOH (l) < H2O(l) < HCN(g) < C2H6(g)

Answer:

Unfavorable reactions include Reaction A and Reaction B.

Favorable coupled reactions: Reactions B with C and Reactions A with C.

Net energy change:

For Reactions B and C: -14.2 kJ/mol

For Reactions A and B: 30.1 kJ/mol

For Reactions A and C: -16.7 kJ/mol

Explanation:

A reaction is considered thermodynamically favorable (or spontaneous) if ΔG is less than 0. Thus, the unfavorable reactions where -ΔG is greater than 0 are:

Reaction A and Reaction B.

In coupling Reaction C with Reaction B and Reaction A, the following equation is obtained:

ATP + fructose-1,6-phosphate ⟶ ADP + fructose-1,6-bisphosphate

ΔG equals 16.3 minus 30.5, resulting in -14.2 kJ/mol.

For the reaction ATP + glucose ⟶ ADP + glucose-6-phosphate, ΔG equals 13.8 minus 30.5, yielding -16.7 kJ/mol.

Overall, the coupled reaction of A and B results in a change of free energy of:

ΔG = 13.8 plus 16.3, which equals 30.1 kJ/mol.