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3 years ago

What is the molarity of a solution made by dissolving 1.25 mol of HCl in enough

Chemistry

1 answer:

Ronch [10]3 years ago

4 0

Answer:

Explanation:

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A sample of nitrogen gas has the temperature drop from 250.°c to 150.°c at constant pressure. what is the final volume if the in

Leviafan [203]

Charles law gives the relationship between temperature of gas and volume of gas.
It states that for a fixed amount of gas, temperature is directly proportional to volume of gas.
V / T = k
where V- volume , T - temperature and k - constant
$\frac{V1}{T1} = \frac{V2}{T2}$
parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation.
T1 = 250 °C + 273 = 523 K
T2 = 150 °C + 273 = 423 K
Substituting the values in the equation,

$\frac{310 mL}{523 K} = \frac{V}{423K}$
V = 251 mL
the new volume is 251 mL

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3 years ago

When 150. g zinc sulfide are burned in excess oxygen, 68.5 g of zinc oxide are actually produced, along with sulfur dioxide. Det

Bumek [7]

%yield = 54.6%

<h3>Further explanation</h3>

Percent yield is the compare of the amount of product obtained from a reaction with the amount you calculated

(theoretical)

General formula:

Percent yield = (Actual yield / theoretical yield )x 100%

<h3 />

Reaction

2ZnS+3O₂ ⇒ 2ZnO+2SO₂

MW ZnS = 97.474 g/mol

mol ZnS

$\tt \dfrac{150}{97.474}=1.54$

MW ZnO = 81.38 g/mol

mol ZnO (from mol ZnS as limiting reactant, O₂ excess)

$\tt \dfrac{2}{2}\times 1.54=1.54$

Actual ZnO produced

$\tt 1.54\times 81.38=125.33~g$

Theoretical production = 125.388

%yield

$\tt \dfrac{68.5}{125.33}\times 100\%=\boxed{\bold{54.6\%}}$

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3 years ago

Balance the following equations

Shtirlitz [24]

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4 years ago

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