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2 years ago

How many moles of hydrogen gas are produced when 0.066 mole of sodium is completely reacted?

Chemistry

2 answers:

velikii [3]2 years ago

8 0

Answer : The number of moles of hydrogen gas is, 0.033 mole

Explanation : Given,

Moles of sodium = 0.066 mole

The balanced chemical reaction will be,

$2Na(s)+2H_2O(l)\rightarrow 2NaOH(aq)+H_2(g)$

From the balanced chemical reaction, we conclude that 2 moles of sodium react with 2 moles of water to give 2 moles of sodium hydroxide and 1 mole of hydrogen has as a product.

As, 2 moles of sodium react to give 1 mole of hydrogen gas

So, 0.066 mole of sodium react to give $\frac{1}{2}\times 0.066=0.033$ moles of hydrogen gas

Therefore, the number of moles of hydrogen gas is, 0.033 mole

SVEN [57.7K]2 years ago

6 0

Base on my research the complete reaction of hydrogen and sodium are form by this equation 2Na + 2H2O = 2NaOH +H2 If we base from this equation it shows you already the ratio of the moles of the product and reactants taking part in the reaction

1 mole of Na r/w 1 mole of water to produce .5 mole of Hydrogen

Therefore, .066 mole of Na produces .033 moles of H2

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AnnyKZ [126]

Answer:

$\large \boxed{1.10 \times 10^{-3}\text{ mol/L}}$

Explanation:

1. Concentration of SO₄²⁻

SrSO₄(s) ⇌ Sr²⁺(aq) +SO₄²⁻(aq); Ksp = 3.44 × 10⁻⁷

0.0150 x

$K_{sp} =\text{[Sr$^{2+}$][SO$_{4}^{2-}$]} = 0.0150x = 3.44 \times 10^{-7}\\x = \dfrac{3.44 \times 10^{-7}}{0.0150} = \mathbf{2.293 \times 10^{-5}} \textbf{ mol/L}$

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x 2.293 × 10⁻⁵

$K_{sp} =\text{[Pb$^{2+}$][SO$_{4}^{2-}$]} = x \times 2.293 \times 10^{-5} = 2.53 \times 10^{-8}\\\\x = \dfrac{2.53 \times 10^{-8}}{2.293 \times 10^{-5}} = \mathbf{1.10 \times 10^{-3}} \textbf{ mol/L}\\\\\text{The concentration of Pb$^{2+}$ is $\large \boxed{\mathbf{1.10 \times 10^{-3}}\textbf{ mol/L}}$}$

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2 years ago

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Reika [66]

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mojhsa [17]

Answer:

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Explanation:

Empirical formula: This is the formula that shows the ratio of elements

present in a

compound.

How to determine Empirical formula

1. First arrange the symbols of the elements present in the compound

alphabetically to determine the real empirical formula. Although, there

are exceptions to this rule, E.g H2So4

2. Divide the percentage composition by the mass number.

3. Then divide through by the smallest number.

4. The resulting answer is the ratio attached to the elements present in

a compound.

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1 1.3

The resulting ratio is 1:1

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