How many moles of hydrogen sulfide are needed to react with sulfur dioxide to produce 1 mole of sulfur?

How many moles of hydrogen sulfide are needed to react with sulfur dioxide to produce 1 mole of sulfur?

2 moles
In order for the reaction to take place, for every mole of sulfur dioxide, you need 2 moles of hydrogen sulfide and produce 3 moles of solid sulfur.

How many moles of O2 react with the available H2S?

1 Expert Answer Proportion 1: 9.3/3=x/2, where 9.3 is the new number of moles of O2, and 3 and 2 are the stoichiometric coefficients of O2 and H2S in the reaction. Solving for x yields that we need 6.2 moles of H2S to use all of the O2.

How many moles of Sulphur will be produced when 2 moles of H2S reacts with 11.2 L of so2 at NTP name the limiting reagent in the above reaction?

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2 mol of ${H_2}S$ 11.2 L $S{O_2}$ at N.T.P. According to this equation 1 mole of $S{O_2}$ reacts with 2 moles of ${H_2}S$. is a limiting agent which is 0.5 moles.

How many grams of sulfur dioxide so2 are formed?

Finally, the mass of sulfur needed to produce four grams of sulfur dioxide is 1.99 grams.

Why is that moles are used for stoichiometric calculations why mass Cannot be used instead?

The answer is because in chemical reactions there is a conservation of moles, rather than mass. Moles are the total amount of molecules in the system, those remain constant. Naturally using numbers like 6.022×1023 is inconvenient, so moles help with keeping track.

When hydrogen sulfide gas H2S reacts with oxygen sulfur dioxide gas and steam are produced?

Problem: When hydrogen sulfide reacts with oxygen, water and sulfur dioxide are produced. The balanced equation for this reaction is: 2H2S (g) + 3O2 (g) → 2H2O (l) + 2SO2 (g) If 9 moles of oxygen react, The reaction consumes _______ moles of hydrogen sulfide.

How many moles of H2O are needed to produce 1 mole of O2 in the following equation?

two moles
Just as before we realize the relationship between water and oxygen by using chemical equation here is two of these to one of these. So we can get these two conversion factors. One mole of O2 to two moles of H2O or two moles of H2O to one mole of O2.

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What bond is SO2?

SO2 is a covalent molecule because the bond is formed between one sulfur and two oxygen atom by the sharing of electrons. Also, the difference of electronegativity between sulfur and oxygen atoms on the Pauling scale is not big enough to make an ionic bond in the SO2 compound.

How is sulfur dioxide formed equation?

When these fuels are burned, the sulfur is oxidised to form sulfur dioxide. S(s) + O 2(g) → SO 2(g) This sulfur dioxide then dissolves in droplets of rainwater to form sulfurous acid.

Why is mole important in stoichiometry?

Quantities of substances can be related to each other using balanced chemical equations. The mole is a key unit in chemistry. Balanced chemical reactions are balanced in terms of moles. A balanced chemical reaction gives equivalences in moles that allow stoichiometry calculations to be performed.

How many moles of sulphur are produced when H2S reacts with SO2?

2 moles of H2S and 11.2 L of SO2 at NTP react to give x mole of sulphur. The Value of ‘x’ will be: Reaction: SO2 (g) + 2H2S (g) → 3S + 2H2O

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What is the molar mass of sulfur dioxide (SO2)?

The sulfur dioxide formula, SO 2, shows that its molecules contain one S atom and two O atoms; calculate its molar mass. One mole SO 2 contains 6.02 x 10 23 SO 2 molecules, which consist of 6.02 x 1023 S atoms and 2(6.02 x 10 23) O atoms. Same for ionic compounds, such as potassium sulfide (K 2 S): 9

What is the oxidation state of sulphur in hydrogen sulfide?

The sulfide in hydrogen sulfide is OXIDIZED (i) to elemental sulfur, and the sulfur dioxide is REDUCED to elemental sulfur…… (ii) Both mass and charge are balanced in each reaction, as indeed they must be if we purport to represent chemical reality…..and so we simply add 2 ×(i) + (ii) to eliminate the electrons to give……..

What is the limiting reagent for hydrogen sulfide and SO2?

And thus SO2 is the limiting reagent and hydrogen sulfide is in excess. And so we gets 3 × an equivalent quantity of S, i.e. 3 ⋅ S 1 ⋅ SO2 × 0.466 ⋅ mols ×32.06 ⋅ g ⋅ mol−1 = 44.8 ⋅ g. And even if you did this reaction carefully in a well-ventilated hood, it would still stink, and the upstairs chemists would come down to give you a beatdown……