Data Given:
Change in Entropy =  ΔH = 120.5 kJ = 1.20 × 10⁵ J

Temperature = T = 298 K

Change in Entropy =  ΔS = 758.2 J/K

Using Formula,
  ΔG =  ΔH - T ΔS
Putting Values,
  ΔG = (1.20 × 10⁵ J) - (298 K × 758.2 J/K)

  ΔG = -1.059 × 10⁵ J

  ΔG = -105.94 kJ

8 0

3 years ago

A cook places a pan of food on a hot stove and leaves it there. When the food is just about done cooking, which of the following

rjkz [21]

Answer:

The pan will be the same temperature as the stove.

Explanation:

7 0

3 years ago

What is the final acetate ion concentration when 69. g Ba(C2H3O2)2 is dissolved in enough water to make 970. mL of solution? The

mario62 [17]

Answer:

0.56M of acetate ions

Explanation:

Given parameters:

Mass of Ba(C₂H₃O₂)₂ = 69g

Volume of water = 970mL = 0.97dm³

Molar mass of Ba(C₂H₃O₂)₂ = 255.415g/mol

Unknown:

Concentration of acetate ion in the final solution = ?

Solution:

Let us represent the dissociation;

Ba(C₂H₃O₂)₂ = Ba²⁺ + 2C₂H₃OO⁻

We see that 1M of will produce 2M of acetate ions

Now, let us find the molarity of the barium acetate;

Molarity = $\frac{number of moles }{volume}$

Number of moles of Ba(C₂H₃O₂)₂ = $\frac{mass}{molar mass}$

Number of moles = $\frac{69}{255.415}$ = 0.27moles

Molarity of Ba(C₂H₃O₂)₂ = $\frac{0.27}{0.97}$ = 0.28M

since 1M of Ba(C₂H₃O₂)₂ will produce 2M of acetate ions

0.28M of Ba(C₂H₃O₂)₂ will produce 2 x 0.28 = 0.56M of acetate ions

3 0

4 years ago