A scientist is examining a mixture of nitrogen, hydrogen, and ammonia. The individual pressures that are exerted by nitrogen and hydrogen are 0.26 atm and 0.28 atm, respectively. If the total pressure is 0.90 atm, what is the partial pressure of ammonia? Use P subscript T equals P subscript 1 plus P subscript 2 plus P subscript 3 plus ellipses plus P subscript n.. 0.27 atm 0.36 atm 0.54 atm 0.90 atm

 0.36 atm

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

Given :   = total pressure of gases = 0.90 atm

= partial pressure of nitrogen =  0.26 atm

= partial pressure of hydrogen = 0.28 atm

= partial pressure of ammonia = ?

putting in the values we get:

Thus the partial pressure of ammonia is 0.36 atm

these nuts

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"