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Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g)...

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Chemistry

Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g) 2H2O(l) + 2 Cl2(g) ΔHrxn = + 96.976 kJ/mol

B.If you place 750 mL of 0.500 M solution of HCl with 17.2 g ofO2, will any oxygen remain? (Hint: limiting reagent problem)

C.What mass of chlorine gas (in grams) is produced?

D) How many molecules of Cl2 are produced based on part (B)

E) What mass of excess reagent remains after the limitingreagent is used up?

F) If the chemist collects 6.98 g of Cl2, what is the percentyield of the reaction? What is the percent error?

G) What is the enthalpy of the reaction for 24.5 g of HCl inpresence of excess O2? Was energy absorbed or released into thesurroundings?

Answer & Explanation Solved by verified expert
3.9 Ratings (363 Votes)
the reaction is 4 HCl 02 2H20 2 Cl2 we know that moles molarity x volume L so moles of HCl 05 x 075 0375 also moles mass molar mass so moles of 02 172 32 05375 now 4 HCl 02 2H20 2 Cl2 moles of 02 required 14 x moles of HCl    See Answer
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