For the reaction below, the thermodynamic equilibrium constant is K= 1.92x103 at 35 °C.NHẠCO2NH2(s) → 2 NH3(g) + CO2(g)Suppose that 0.0046 moles of NHẠCO2NH2, 0.0092 moles of NH3, and 0.0046 moles of CO2 are added to a 3.00 Lcontainer at 35 °C.(a) What are Q and A,G for the initial reaction mixture? Your answers must be accurate to 3 significant figures.Q = NumberA,G= NumberkJ mol-1(b) Is the spontaneous reaction to the left or to the right?Click for List

Given : We have to tell Q and delta G of the reaction.

or the reaction below, the thermodynamic equilibrium constant is K= 1.92×10-3 at 35 °C. H4CO2NH2(s) – 2 NH3(g) + CO2(g) uppose that 0.0046 moles of NHĄCO2NH2, 0.0092 moles of NH3, and 0.0046 moles of CO2 are added to a ontainer at 35 °C. ) What are Q and A,G for the initial reaction mixture? Your answers must be accurate to 3 significant fi Q = Number A;G= Number kJ mol-1 ) Is the spontaneous reaction to the left or to the right? Click for List

or the reaction below, the thermodynamic equilibrium constant is K= 1.92×10-3 at 35 °C. H4CO2NH2(s) – 2 NH3(g) + CO2(g) uppose that 0.0046 moles of NHĄCO2NH2, 0.0092 moles of NH3, and 0.0046 moles of CO2 are added to a ontainer at 35 °C. ) What are Q and A,G for the initial reaction mixture? Your answers must be accurate to 3 significant fi Q = Number A;G= Number kJ mol-1 ) Is the spontaneous reaction to the left or to the right? Click for List

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 80QRT

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