Consider the following unbalanced chemical equation. H2S(g) + O2(g) → SO2(g) + H2O(g) Determine the maximum...

Question

Question

Consider the following unbalanced chemical equation.

H₂S(g) + O₂(g) → SO₂(g) + H₂O(g)

Determine the maximum number of moles of SO₂ produced from 10.0 moles of H₂S and 4.00 moles of O₂.

Answer 1

Answer #1

но) +ts) - se) +ңos) balanced equation is 2ңS (s) + го созно + 2 so - по шва е цѕ a look no. gudler of a = 4:00ust - зо - а.а

Answer 2

Similar Homework Help Questions

Consider the following unbalanced chemical equation H2S(g)+O2(g)=SO2(g)+H2O(g) Determine the maximum number of moles of SO2 produced...

Consider the following unbalanced chemical equation H2S(g)+O2(g)=SO2(g)+H2O(g) Determine the maximum number of moles of SO2 produced from 10.00 moles H2S and 5.00moles of O2
4. Balance the following chemical reaction: H2S(0) + O2(g) → SO2(g) + H2O

4. Balance the following chemical reaction: H2S(0) + O2(g) → SO2(g) + H2O
Consider the following reaction: 2 H2O(g) + 2 SO2(g) ↔ 2 H2S(g) + 3 O2(g) A...

Consider the following reaction: 2 H2O(g) + 2 SO2(g) ↔ 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6. Consider the following reaction: 2 H2O(g) + 2 SO2(g) ↔ 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc...

Consider the following balanced chemical equation: 2H2S(g) + SO2(g) → 3S(s) + 2H2O(g) a. How many...

Consider the following balanced chemical equation: 2H2S(g) + SO2(g) → 3S(s) + 2H2O(g) a. How many moles of H2S must react to form 4.18 moles of S? _ moles H2S b. How many moles of SO2 must react to form 4.18 moles of S? _ moles SO2 c. How many moles of H2S must react to form 4.18 moles of H2O? _ moles H2S d. How many moles of SO2 must react to form 4.18 moles of H2O? _ moles...
Consider the following unbalanced equation: O2(g) + C4H10(g) → CO2(g) + H2O(l) If 3.56×102 moles of...

Consider the following unbalanced equation: O2(g) + C4H10(g) → CO2(g) + H2O(l) If 3.56×102 moles of O2(g) and 47.3 moles of C4H10(g) are allowed to react to produce 1.10×102 moles of CO2(g), what is the percent yield of the reaction? 29.2% 58.1% 89.5% 89.9% 65.7%
Consider the following unbalanced chemical equation. C5H12(/) + 02(g) → CO2(g) + H2O(/) If 37.2 grams...

Consider the following unbalanced chemical equation. C5H12(/) + 02(g) → CO2(g) + H2O(/) If 37.2 grams of pentane (CH12) are burned in excess oxygen, how many grams of H20 will be produced? g H20

Consider the following reaction: SO2 + 2 H2S → 3 S + 2 H2O If 7.40...

Consider the following reaction: SO2 + 2 H2S → 3 S + 2 H2O If 7.40 g of SO2 reacts via this reaction in excess H2S, what mass (in g) of H2O will be produced?
Consider the unbalanced equation for the following reaction: O2(g) + C6H5COOH(aq) → CO2(g) + H2O(l) If...

Consider the unbalanced equation for the following reaction: O2(g) + C6H5COOH(aq) → CO2(g) + H2O(l) If 54.0 grams of C6H5COOH(aq) reacts with an excess of O2(g) and 103. grams of CO2(g) is formed, determine the percent yield of CO2(g). (the answer is 76.0%, I want to know the process)
consider the unbalanced equation for the following reaction O2(g) + C3H8 Reviewing Pool 4 Question 1...

consider the unbalanced equation for the following reaction O2(g) + C3H8 Reviewing Pool 4 Question 1 Available Point 10 Consider the unbalanced equation for the following reaction Oxg) -CH() - COX). How Determine the amount of H2O(l) formed in the reaction if 9.50 moles of OC reacts with an excess of C ) and the percent yield of Ho %

Consider the unbalanced equation for the combustion of hexane: aC6H14(g) + BO2(g) +7CO2(g) + H2O(g) Determine...

Consider the unbalanced equation for the combustion of hexane: aC6H14(g) + BO2(g) +7CO2(g) + H2O(g) Determine how many moles of O2 are required to react completely with 5.8 mol of C6H14. Express your answer using two significant figures. View Available Hint(s) ΨΗ ΑΣΦ ] ? n = mol Submit