Arcylonitrile, c3h3n, is the starting material for the production of a synthetic fiber and can be made from propylene, c3h6, reacting with nitrogen monoxide, no, as follows: 4 c3h6 (g) + 6 no (g) → 4 c3h3n (s)+ 6 h2o (l) + n2 (g) how many moles of acrylonitrile are formed when 5.0 moles of propylene reacts with 9.0 moles of nitrogen monoxide?

              5 moles of C₃H₃N

The Balance Chemical Equation is as follow,

                           4 C₃H₆ + 6 NO        →      4 C₃H₃N  +  6 H₂O + N₂

Step 1: Calculate the Limiting Reagent,

According to Balance equation,

               4 moles of C₃H₆ reacts with  =  6 moles of NO

So,

                   5 moles of C₃H₆ will react with  =  X moles of NO

Solving for X,

                       X  =  (5 mol × 6 mol) ÷ 4 mol

                       X  =  7.5 mol of NO

It means 5 mol of C₃H₆ requires 7.5 mol of NO, while we are provided with 9 mol NO which is in excess. Therefore, C₃H₆ is the limiting reagent and will control the yield of products.

Step 2: Calculate amount of C₃H₃N produced,

According to equation,

                4 moles of C₃H₆ produces  =  4 moles of C₃H₃N

So,

                        5 moles of C₃H₆ will produce  =  X moles of C₃H₃N

Solving for X,

                      X  =  (5 mol × 4 mol) ÷ 4 mol

                      X  =  5 moles of C₃H₃N

im not exactly sure but i think its b!

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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