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Suppose you are performing a gas-producing reaction with an unknown metal, X . X ( s ) + 2 H C l ( a q ) ⟶ X C l 2 ( a q ) + H 2 ( g ) A sample of 0.243 g of the unknown metal produces 76.9 mL of H 2 gas. The gas is collected over water at an atmospheric pressure of 768.3 mm Hg at 23 oC, at which the vapor pressure of water is 21.1 mm Hg. Assume that the hydrogen gas behaves ideally. What is the experimental value for the molar mass of the metal in g/mol?

Respuesta :

Answer:

600,000,000,000,000,000

Explanation:

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The experimental value for the molar mass of the metal in g/mol is 78.14 g/mol

How to determine the mole of hydrogen collected

  • Volume (V) = 76.9 mL = 76.9 /1000 = 0.0769 L
  • Temperature (T) = 23 ˚C = 23 + 273 = 296 K
  • Pressure (P) = 768.3 – 21.1 = 747.2 mmHg = 747.2 / 760 = 0.983 atm
  • Gas constant (R) = 0.0821 atm.L/Kmol
  • Number of mole (n) =?

The number of mole can be obtained by using the ideal gas equation as illustrated below:

n = PV / RT

n = (0.983 × 0.0769) / (0.0821 × 296)

n = 0.00311 mole

How to determine the molar mass of the metal

Balanced equation

X + 2HCl —> XCl₂ + H₂

From the balanced equation above,

1 mole of H₂ was obtained from 1 mole of X.

Therefore,

0.00311 mole of H₂ will also be obtained from 0.00311 mole of X

Thus, we can obtain the molar mass of the Metal X as follow:

  • Mass of X = 0.243 g
  • Mole of X = 0.00311 mole
  • Molar mass of X =?

Molar mass = mass / mole

Molar mass of X = 0.243 / 0.00311

Molar mass of X = 78.14 g/mol

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