At 500 °C, hydrogen iodide decomposes according to 2 HI ( g ) − ⇀ ↽ − H 2 ( g ) + I 2 ( g ) For HI ( g ) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [ H 2 ] = 0.335 M , [ I 2 ] = 0.335 M , and [ HI ] = 2.83 M . If an additional 1.00 mol of HI ( g ) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached?

What is impossible to do with a hypothesis

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

How do you convert 4 mmol of bromobenzene to ml?