What mass of hydrogen sulfide, H2S, will completely react with 2.00 moles of silver nitrate, AgNO3?

2AgNO3 (aq) + H2S (aq)
Ag2S (s) + 2HNO3 (aq)

17.0 g H2S (aq)
34.1 g H2S (aq)
46.3 g H2S (aq)
64.2 g H2S (aq)

Question

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Respuesta :

apradhan49 apradhan49 · Answer 1 · 2021-02-26T21:19:19+01:00

Answer:

34g

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

H2S + 2AgNO3 —> 2HNO3 + Ag2S

Next, we shall determine the number of mole of H2S required to react with 2 moles of AgNO3.

This is illustrated below:

From the balanced equation above,

We can see that 1 mole of H2S is required to react completely with 2 moles of AgNO3.

Finally, we shall convert 1 mole of H2S to grams. This is shown below:

Number of mole H2S = 1 mole

Molar mass of H2S = (2x1) + 32 = 34g/mol

Mass = number of mole x molar Mass

Mass of H2S = 1 x 34

Mass of H2S = 34g

Therefore, 34g of H2S is needed to react with 2 moles of AgNO3.

dsdrajlin dsdrajlin · Answer 2 · 2022-02-04T13:10:33+01:00

2.00 moles of AgNO₃(aq) react completely with 34.1 g of H₂S(aq).

Let's consider the following balanced equation.

2 AgNO₃(aq) + H₂S(aq) ⇒ Ag₂S(s) + 2 HNO₃(aq)

We want to calculate the mass of H₂S required to completely react with 2.00 moles of AgNO₃. This is a stoichiometry problem.

Stoichiometry is the relationship between the relative quantities of substances taking part in a reaction or forming a compound.

To calculate the mass of H₂S, we need to consider the following relationships.

[tex]2.00molAgNO_3 \times \frac{1molH_2S}{2molAgNO_3} \times \frac{34.1gH_2S}{1molH_2S} = 34.1 g H_2S[/tex]

2.00 moles of AgNO₃(aq) react completely with 34.1 g of H₂S(aq).

Learn more about stoichiometry here: https://brainly.com/question/16060223