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marishachu [46]
3 years ago
11

he equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture o

f the three compounds in a 4.90 L container at 673 K contains 1.45 mol of NH4I(s) and 0.405 mol of NH3, the number of moles of HI present is moles.
Chemistry
1 answer:
frosja888 [35]3 years ago
3 0

<u>Answer:</u> The number of moles of HI in the solution is 1.24\times 10{-3} moles.

<u>Explanation:</u>

We are given:

K_c=7.00\times 10^{-5}\\n_{NH_3}=0.405mol\\n_{NH_4I}=1.45mol\\V=4.90L

To calculate the concentration of a substance, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}     ......(1)

  • Concentration of ammonia:

[NH_3]=\frac{0.405mol}{4.90L}=0.083mol/L

  • Concentration of ammonium iodide:

[NH_4I]=\frac{1.45mol}{4.90L}=0.30mol/L

For the given chemical reaction:

NH_4I(s)\rightleftharpoons NH_3(g)+HI(g)

The expression of K_c for above equation follows:

K_c=\frac{[HI][NH_3]}{[NH_4I]}

Putting values in above equation, we get:

7.0\times 10^{-5}=\frac{[HI]\times 0.083}{0.30}

[HI]=2.53\times 10^{-4}

Calculating the moles of hydrogen iodide by using equation 1, we get:

2.53\times 10^{-5}=\frac{\text{Moles of HI}}{4.9}\\\\\text{Moles of HI}=1.24\times 10^{-3}

Hence, the number of moles of HI in the solution is 1.24\times 10{-3} moles.

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3 years ago
Salt is often added to water to raise the boiling point to heat food more quickly. if you add 30.0g of salt to 3.75kg of water,
sammy [17]

Assuming an ebullioscopic constant of 0.512 °C/m for the water, If you add 30.0g of salt to 3.75kg of water, the boiling-point elevation will be 0.140 °C and the boiling-point of the solution will be 100.14 °C.

<h3>What is the boiling-point elevation?</h3>

Boiling-point elevation describes the phenomenon that the boiling point of a liquid will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent.

  • Step 1: Calculate the molality of the solution.

We will use the definition of molality.

b = mass solute / molar mass solute × kg solvent

b = 30.0 g / (58.44 g/mol) × 3.75 kg = 0.137 m

  • Step 2: Calculate the boiling-point elevation.

We will use the following expression.

ΔT = Kb × m × i

ΔT = 0.512 °C/m × 0.137 m × 2 = 0.140 °C

where

  • ΔT is the boiling-point elevation
  • Kb is the ebullioscopic constant.
  • b is the molality.
  • i is the Van't Hoff factor (i = 2 for NaCl).

The normal boiling-point for water is 100 °C. The boiling-point of the solution will be:

100 °C + 0.140 °C = 100.14 °C

Assuming an ebullioscopic constant of 0.512 °C/m for the water, If you add 30.0g of salt to 3.75kg of water, the boiling-point elevation will be 0.140 °C and the boiling-point of the solution will be 100.14 °C.

Learn more about boiling-point elevation here: brainly.com/question/4206205

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Answer:

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Explanation:

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