The system co2(g) + h2(g) ⇀↽ h2o(g) + co(g) is at equilibrium at some temperature. at equilibrium a 4.00 l vessel contains 1.00 mole co2, 1.00 mole h2, 2.40 moles h2o, and 2.40 moles co. how many moles of co2 must be added to the system to bring the equilibrium co concentration to 0.791 mol/l? answer in units of moles.

The equilibrium expression for this reaction is'      the question says that at equilibrium, those molecules have those concentrations. therefore, we can calculate the values.if concentration is in mol/l, and the vessel is 4.00 l, then we can calculate the equilibrium concentrations of each:         and thus, the equilibrium constant for this reaction is      the equilibrium constant is 5.76.now, let x be added concentration of co₂.we can convert to moles after to answer the question.when we add, a new equilibrium is formed.so we make an ice table, as shown in the diagram.initially, we have the original concentrations of all the reactants and products, except with  co₂ because we're adding on to that.we want the equilibrium co to be 0.791 m, so we indicate that by placing 0.791 in the e row for co.the explanation in the diagram should suffice for the next steps.the equilibrium constant for this new equilibrium is    but we know that  the equilibrium constant has a value of 5.76.  the equilibrium constant only changes if the temperature is changed.so keq should also be 5.76. now we can solve for x.i distribute 0.059 into the parentheses.    multiply both sides by the denominator so that the denominator on the right side gets canceled out.    subtracting both sides by  , we obtain    dividing both sides by  , we obtain    we have x=1.78 msince x represents concentration, convert to moles.    have to add 7.12 moles of co2.

1. and 2. question: in which equation? or i don't understand you, 3. a), 4. c), 5. c), 6. b), 7. d), 8. d) if small number is underlined(behind symbol) , b) if big number is underlined(in front of symbol)9. what is underlined there? 10. c)

The answer to this problem is. 67