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3 years ago

4. Given the balanced equation: 2Na + S → Na₂S

Chemistry

1 answer:

PtichkaEL [24]3 years ago

8 0

Answer:

Option D. 30 g

Explanation:

The balanced equation for the reaction is given below:

2Na + S —> Na₂S

Next, we shall determine the masses of Na and S that reacted from the balanced equation. This is can be obtained as:

Molar mass of Na = 23 g/mol

Mass of Na from the balanced equation = 2 × 23 = 46 g

Molar mass of S = 32 g/mol

Mass of S from the balanced equation = 1 × 32 = 32 g

SUMMARY:

From the balanced equation above,

46 g of Na reacted with 32 g of S.

Finally, we shall determine the mass sulphur, S needed to react with 43 g of sodium, Na. This can be obtained as follow:

From the balanced equation above,

46 g of Na reacted with 32 g of S.

Therefore, 43 g of Na will react with = (43 × 32)/46 = 30 g of S.

Thus, 30 g of S is needed for the reaction.

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A 25.0 ml sample of 0.150 m hydrazoic acid is titrated with a 0.150 m naoh solution. what is the ph after 15.0 ml of the sodium

babunello [35]

First, we need to calculate moles of hydrazoic acid NH3:

moles NH3 = molarity * volume

= 0.15 m * 0.025 L

= 0.00375 moles

moles NaOH = molarity * volume

= 0.15 m * 0.015 L

= 0.00225 moles

after that we shoul get the total volume = 0.025L + 0.015L

= 0.04 L

So we can get the concentration of NH3 & NaOH by:

∴[NH3] = moles NH3 / total volume

= 0.00375 moles / 0.04 L

= 0.09375 M

∴[NaOH] = moles NaOH / total volume

= 0.00225 moles / 0.04 L

= 0.05625 M

then, when we have the value of Ka of NH3 so we can get the Pka value from:

Pka = -㏒Ka

= - ㏒ 1.9 x10^-5

= 4.7

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3 years ago

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It makes it more accessible to everybody

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3 years ago

Classify the following as homogeneous or heterogeneous mixtures, or pure

victus00 [196]

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3 years ago

Suppose of hcl and of o2 are added to an empty flask. How much will be in the flask at equilibrium?A. None. B. Some, but less th

serg [7]

This is an incomplete question, here is a complete question.

Hydrogen chloride and oxygen react to form water and chlorine, like this:

$4HCI(g)+O_2(g)\rightarrow 2H_2(g)+2CI_2(g)$

Use this chemical equation to answer the questions in the table below.

Suppose 155. mmol of HCl and 38.8 mmol of O₂ are added to an empty flask. How much HCl will be in the flask at equilibrium?

(1) None.

(2) Some, but less than 155. mmol,

(3) 155. mmol,

(4) More than 155. mmol,

Answer : The correct option is, (1) None

Explanation :

The given balanced chemical reaction is:

$4HCI(g)+O_2(g)\rightarrow 2H_2(g)+2CI_2(g)$

From the balanced chemical reaction, we conclude that

As, 4 mmole of HCl react with 1 mmoles of $O_2$

So, 155. mmole of HCl react with $\frac{155.}{4}\times 1=38.75$ mmoles of $O_2$

That means, $O_2$ is excess reagent and $HCl$ is a limiting reagent. All the moles of HCl will consume.

Hence, the correct option is, None.

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3 years ago