Problem: Ammonium carbamate (NH2COONH4) is a salt of carbamic acid that is found in the blood and urine of mammals. At 250°C, Kc = 1.58 x 10−8 for the following equilibrium:   NH2COONH4(s) ⇌ 2NH3(g) + CO2(g) If 7.80 g of NH2COONH4 is put into a 0.500-L evacuated container, what is the total pressure at equilibrium?

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Ammonium carbamate (NH2COONH4) is a salt of carbamic acid that is found in the blood and urine of mammals. At 250°C, Kc = 1.58 x 10−8 for the following equilibrium:   

NH2COONH4(s) ⇌ 2NH3(g) + CO2(g) 

If 7.80 g of NH2COONH4 is put into a 0.500-L evacuated container, what is the total pressure at equilibrium?