Struggling with setting up the table for part B. Nitrosyl bromide (NOBr) can be

Question

Struggling with setting up the table for part B.

Nitrosyl bromide (NOBr) can be obtained as a pure liquid at low temperatures. The liquid boils at -2degree C, and at room temperature the gas partially decomposes, as shown below. 2 NOBr(g) A 2.00-g sample of cold liquid NOBr is injected into a 1.0 L flask. (Assume that the flask was first evacuated so that it does not contain any air or other gases.) When the flask is allowed to come to equilibrium at 298 K, the total pressure inside is measured as 0.624 atm. Calculate the total number of moles of gas present in the flask at equilibrium. (This part should be easy!) (b). Now find the numerical value of K_eq for the reaction above at 298 K.

Explanation / Answer

2NOBr ------------> 2NO + Br2

Find the equilibrium concentrations of NOBr, NO ,  Br2

Keq = concentration of products at equilibrium/ concentration of reactants at equilibrium

Keq = [NO]2 [Br2] / [NOBr]

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