If a sample of 0.500 moles of hydrogen sulfide H₂S was reacted with excess concentrated sulfuric acid then, number of moles of sulfur dioxide SO₂ would be produced are 2.00.
It is the ratio of mass of element in grams of a given compound and the molar mass of the element. In order to have balanced equation, we have to find the correct number of mole of SO₂. The reaction is
H₂S(g) + 3H₂SO₄ ⇄ 4H₂O(l) + 4SO₂
1 mole of H₂S react with excess of H₂SO₄ to give 4 moles of SO₂.
0.5 mole of H₂S react with excess of H₂SO₄ to give 4 x 0.5 =2.00 moles of SO₂.
Thus, 2 moles of sulfur dioxide SO₂ would be produced.
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