Ammonium carbamate (nh2coonh4) is a salt of carbamic acid that is found in the blood and urine of mammals. at 202°c, kc = 0.008 for the following equilibrium: if 6.82 g of nh2coonh4 is put into a 0.5-l evacuated container, what is the total pressure (in atm) at equilibrium? enter a number to 2 decimal places.

P(total) = 46.08 atm

Explanation:

Given data:

Mass of NH₂COONH₄ = 6.8 g

Kc = 0.008

Temperature = 202°C = 202+273 = 475 K

Total pressure at equilibrium = ?

Solution:

Equilibrium equation:

NH₂COONH₄   ⇄   2NH₃ + CO₂

Formula:

Kp = Kc(RT)³

Kp = 0.008 (0.0821 atm.L/mol.K )³(475K)³

Kp = 471.56

                                                                  NH₃       CO₂

            Initial concentration                       0          0

            Change in concentration             2x           x

            equilibrium concentration            2x           x

AS

471.56 = 2x (x)

471.56 = 2x²

x² = 471.56 /2

x² = 235.78

x = 15.36

Pressure of ammonia = 2x = 2(15.36) = 30.72 atm

Pressure of carbon dioxide = x = 15.36 atm

Total pressure:

P(total) = P(NH₃) + P(CO₂)

P(total) = 30.72 atm +  15.36 atm

P(total) = 46.08 atm

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: