Consider the reaction. 2A(g)↽−−⇀B(g)p=7.84×10−5at 500 K

If a sample of A(g) at 1.90 atm is heated to 500 K, what is the pressure of B(g) at equilibrium?

B=
atm

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Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4nh3 (g) + 5o2 (g) → 4no (g) + 6h2o (g) also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium nh3 65.1atm o2 31.3atm no 62.7atm h2o 65.8atm compound pressure at equilibrium nh3 65.3 atm o2 7.79 atm no 12.1 atm h2o 65.8 atm calculate the value of the equilibrium constant kp for this reaction. round your answer to 2 significant

Hey guys so i need to know what is _nh3+> nh4oh ~chemistry~