Question

A reaction occurs between ammonia and carbon dioxide in the following chemical reaction: 2NH, + CO2 → (NH2)2CO + H2O In the process, 637.2 g of NH, are treated with 1142 g of CO. Calculate the percert yield if 1000. g of (NHa) CO are actually obtained.

Answer 1

No. oF Moles: mas S (m) Moles (n) molay mass (M) Limitinq Reactant: a . chemical reaction The工imiting veagent Con sumed whe n the the Subs tonce thal totally reactioComplete. The amount o reaqent,Since the reaction Chemical product formed )imited Cannot Continue by this wi thout . it Percent Yield; Percent Yeld the Percent ratio actual yield to łhe the 0 e t i cal yield actual Yield Percent Yield x 100>. Theoreticat Yield

CalcWate percent Yield: Finding the limi ting veactant: Hass吋NH3-637.29- - 17.031 /mol a f moles mass ..63 7.2q 3 molar mass 17.031 J/mo l Molar MaSS吋C02-44.013/mol No.oj moles ซึ่ -mass 42 3 44 019Imol 2 5.949 mol CO2 molay mass .-. Co2 i the limiting veactant I mol (NH2) 2co 25.949 mo) (NH2), co Mo les Molar Mass oj nH)2 cD Mass 吋(NH2)2C0 = moles× molar mass 6 0, 0 553 /no l 25.94mol x60. oss3 9/mol : iss8 .37 (NH2)2CO Theove tical Yield - 558.37g 4V)1cto Percent Yield Percent Yield-Actual vieid 100 . Theoret ical Yieid o 0 0 9 I558.37 & 0.6417 x l00X. : 64.17 % Percent yield of aHa), co -C4m17