13. 3/4 points | Previous Arswers My Notes AskYour Nitric oxide and bromine at i

Question

13. 3/4 points | Previous Arswers My Notes AskYour Nitric oxide and bromine at intial pressures is as follows. of 98.4 and 41.3 tor, respectively, were allowed to react at 300K. At equilibrium the total pressure was 110.5 torr. The reaction 2 N0(g) + Br2(g)-2 NOBr(0) (a) Calculate the value of Kp 132 (b) What would be the partial pressures of all the species if NO and Bra, both at an initial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature? PNo 00268 atm Par2 176 PoB 248atm Need Help? Read 3/6 points| Phevious Answers ZumChem10 13.E.116 My Notes Aak Your Tesc

Explanation / Answer

I see you have found the kp = 132, i will focus on the second problem

so you have to do an ice Chart

Reaction is

.................2 NO + Br2 ========= 2NOBr

I.................0.3.......0.3.........................0

C...............-2x.........-x.........................+2x

E..............0.3-2x.....0.3-x......................2x

partial pressure of NO is 0.3 - 2x

partial pressure of Br2 is 0.3 - x

partial pressure of NOBr is 2x

For the equilibrium constant remember that it is the ratio of pressure of products to pressure of reactants

kp = 2x2 / [0.3-2x]2[0.3-x] = 132

if you solve this equation you will find a value of x equal to 0.124 atm

so partial pressure of NO is

0.3 - 2*(0.124) = 0.0515 atm

partial pressure of Br2

0.3 - 0.124= 0.17578 atm

parital pressure of NOBr

2*0.124 = 0.248 atm

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