Question

pts) Consider the following balanced equation: Na2SO4 (aq) + 2AgNO3 (aq) → Ag2SO4 (9) + 2NaNO3(aq) a. How many grams of Ag2SO4 result from the reaction of 6.764 g of Na SO, with 15.00 g of AgNO3? b. If the reaction has a 57.3% percent yield, how much Ag2SO4 was actually made? pts) How many grams of O, reacted if 306 kcal are released in the following reaction? CH(g) + 2O2(g) - CO2(g) + 2H2O(l) + 213 kcal

Answer 1

Na₂SO4 ou + 2 AgNO3 609) Imole amoles Ag₂SO4 (s, t & NaNogans imole a moles One mole of Nasoy neact with two moles of Agasoy. produce AgNO3 to one mole of I mole of Nasoy : 143.04g 6.764 g of Nag soy = 6.764 more: 0.04762 mole 142.04 Imole of AgNO3 = 169.8729 15 g of AgriO₂ = 1 = 0. 0883 mole

0.04762 mole of Hagsly need (2x0.04762) mole of AgNO₃ to react. That is 0.09524 mole. But AgNO3 priesent is 0.0883 mole. That is in less quantity. so. Agniuz limiting agent. 0.0883 mole of Agnio, neart with (0.0883) mole of Nasoy. That is 0.04415 mole of Masson. one mole of Nasoy produce one mole Agasan 0.04415 more of Na, soy produce 0.04415 mole of Agasoy. Imole of Age soy = 311.799 g. 0.04 415 mole of Aga Soy = 0.04415*311.799 = /13.776 g of Agasoy (Ans) Theoritical yeild = /13.776 g of Aga soy (100% yield) (b) 96 57.3% yield then, actual yield in gram. 13.776* 573 - (7.894 grom (Ans)