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VladimirAG [237]
3 years ago
10

Last week you reacted magnesium with a hydrochloric acid aqueous solution and hydrogen gas was produced. Let's say that you coll

ected the gas given off by the reaction and measured it's pressure as 101.2 kPa. If the vapor pressure of water is 31.4 kPa at this temperature, then what is the pressure of the hydrogen gas?
Chemistry
1 answer:
miv72 [106K]3 years ago
3 0

Answer:

69.8 kilo Pasacl is the pressure of the hydrogen gas.

Explanation:

Mg+2HCl\rightarrow MgCl_2+H_2

Pressure at which hydrogen gas collected = p = 101.2 kilo Pascals

Vapor pressure water = p^o = 31.4 kilo Pascals

The pressure of hydrogen gas = P

The pressure at which gas was collected was sum of vapor pressure of water and hydrogen gas.

p=P+p^o

P =p-p^o=101.2 kPa-31.4 kPa=69.8 kPa

69.8 kilo Pasacl is the pressure of the hydrogen gas.

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Answer:

5.2 x 10⁻⁴ M.

Explanation:

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<em>P = kC</em>

where P is the partial pressure of the gaseous  solute above the solution.

k is a constant (Henry’s constant).

C is the concentration of the dissolved gas.

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<em>P₁C₂ = P₂C₁,</em>

P₁ = 1.0 atm, C₁ = 6.8 x 10⁻⁴ mol/L.

P₂ = 0.76 atm, C₂ = ??? mol/L.

<em>∴ C₂ = (P₂C₁)/P₁ =</em> (0.76 atm)(6.8 x 10⁻⁴ mol/L)/(1.0 atm) = <em>5.168 x 10⁻⁴ mol/L ≅ 5.2 x 10⁻⁴ M.</em>

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7 0
3 years ago
How much ch2o is needed to prepare 445 ml of a 2.65 m solution of ch2o?
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Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

Molarity=\frac{n\times 1000}{V_s}

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Putting in the values we get:

2.65=\frac{n\times 1000}{445ml}

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Mass of solute in g=moles\times {\text {molar mass}}=1.18mol\times 30.02g/mol=35.4g

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