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Westkost [7]
2 years ago
12

Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s−1 .

Chemistry
1 answer:
katrin [286]2 years ago
4 0
The correct is this because they said
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When magnesium chloride reacts with water, 5.85 L HCl(g) is produced.
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Answer: How many moles of HCl was produced?

⇒ 0.261 moles of HCl

How many moles of MgCl2 reacted?

⇒ 0.131 moles of MgCl2

What mass of MgCl2 reacted?

⇒ 12.4 g MgCl2

Explanation:

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Which group has elements with the most diverse set of properties??
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Group 4A

The elements in group 4 show the most diverse set of properties.
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A 2.350×10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then b
sveta [45]

Answer:

  • Part A: m = 0.02356 mol/kg = 0.02356 m
  • Part B: Xsolute = 4.243×10⁻⁴
  • Part C: % m/m = 0.1376%
  • Part D: ppm = 1,376 ppm

Explanation:

<u>1. Data:</u>

a) M = 2.350×10⁻² M

b) V sol = 1.000 L

c) V H₂O = 994.4 mL = 0.9944 L

d) d H₂O = 0.9982 g/mL

<u>2. Formulae</u>

  • M = n solute / V sol (L)
  • m = n solute / Kg solvent
  • X solute = n solute / N total
  • % m/m = (mass of solute / mass of solution) × 100
  • ppm = (mass of solute / mass of solution) × 1,000,000
  • density = mass in grams / volume in mL

<u>3. Solution</u>

<u>Part A: Calculate the molality of the salt solution. </u>

<u />

            m = n solute / Kg solvent

i) M = n solute / V sol (L) ⇒ n solute = M × V sol (L)

⇒ n solute = M = 2.350×10⁻² M × 1.000 L = M = 2.350×10⁻² mol

ii) density H₂O = mass H₂O / volume H₂O

⇒ mass H₂O = density H₂O × volume H₂O

⇒ mass H₂O = 0.9982 g/mL × 999.4 mL = 997.6 g

iii) kg  H₂O = 997.6 g / (1,000 g/Kg) = 0.9976 kg

iv) m = 2.350×10⁻² mol / 0.9976 kg = 0.02356 mol/kg = 0.02356 m

<u>Part B: Calculate the mole fraction of salt in this solution</u>.

          X solute = n solute / N total

i) n solute =  2.350×10⁻² mol

ii) n solvent = n H₂O = mass H₂O in grams/ molar mass H₂O

⇒ 997.6 g / 18.015 g/mol = 55.38 mol

iii) X solute = 2.350×10⁻² mol / 55.38 mol = 4.243×10⁻⁴

<u>Part C: Calculate the concentration of the salt solution in percent by mass</u>.

         % m/m = (mass of solute / mass of solution) × 100

i) molar mass = mass in grams / molar mass

⇒ mass of solute = mass of NaCl = n solute × molar mass NaCl

⇒ mass of solute = 2.350×10⁻² mol × 58.44 g/mol = 1.373 g

ii) % m/m = (1.373 g / 997.6 g) × 100 = 0.1376%

Part D: Calculate the concentration of the salt solution in parts per million.

       ppm = (mass of solute / mass of solution) × 1,000,000

i) ppm = ( (1.373 g / 997.6 g) × 1,000,000 = 1,376 ppm

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Physical or Chemical Change? Burning leaves
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