Question

1. Gaseous NO reacts with oxygen gas to make gaseous nitrogen dioxide. Initially NO and oxygen as separated as shown below. When the valve is opened, the reaction quickly goes to completion. Assume that the temperature remains constant at 35°C. This quiz will sort of walk you through the calculations involved to determine the pressure in the now connected flasks after the completion of the reaction. after valve opened BEFORE REACTION before valve opened NO (g) O2 (g) 1.75 atm 0.600 atm 3.50 L 1.50 L Diagram B Diagram A a) Briefly but clearly explain why the pressure in diagram B is NOT 2.35 atm. The diagram Pressure equal to the tuo pressures added ,not subtracted b) Calculate the partial pressure of NO after the valve is opened but before any reaction (diagram B)? Calculate the partial pressure of O2 after the valve is opened but before any reaction (diagram B)? c) d) Calculate the total pressure in the container after the after the valve is opened but before any reaction (in diagram B)? O

Answer 1

@ Pressure in diagram B is not 2.35 atm Itisdue after value is opened and before reaction. The volume of the gases changes from 1.50L of No to 5.0L and same way 3.50L of 02 90s changed to 50L if volume increases the pressure of each goses decreases so the Pressure should not be 175 atm to 600 atm = 2.35atm. And after reaction number of moles of gas changes so pressure is not 2:35ath 6 since temprature is constant partial pressure of no be calculated with formula P v = Pave before reaction P= Initial pressure of No = 1.75aling v= volume of No Initial=1.50L - Final Pressure of NOx ; Vg = Final volume @ No: since the value is opend total volume will final volumso Final volumed NO (V2) = 1-50L +3.50L = 5.00L Final Pressure & Partial Pressure of No (P2) = PIVI in = 1.75atm X 1-50% -0.525atm of No 5.004 I Initial volume of c l = 3.504, Initial volumes Final volume of Oz (vel= 5:00h, Final pressure of C (Pal= x Fural Pression by partial pressure calle) = Partial pressure of op[P2)0.6ocalmx 3.500 0.42 atm According Dalton's law 500x Total pussue = Paxtial pressured 02+ partial pressure of No = 0.52atm to. 42atm = 0.945 atm All above calculations havebeen done before reaction start between No and a goses. Total Pressure of Container after value is opend before reaction 0.945 atm Ve Partial pressure Presoule Pil -0. Goocture