||| Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL. flask is filled with 1.6 mol of CO, 0.90 mol of H₂O and 1.4 mol of H₂. The following reaction becomes possible: Co(g) +H₂O(g) CO₂(g) +H₂(g) The equilibrium constant K for this reaction is 7.19 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. 8 M X 3

When using a calibration curve and beers law if one of your a diluted test solutions had an absorbance greater than the calibration range. Why is that value disregarded?

This is actually question from past paper and I really need to answer for theses question

A calibration curve was created to determine the quantity of protein in a solution. The calibration curve has the form of a straight line with the equation ?=0.0182?+0.007 where ? is the corrected absorbance of the solution and ? is quantity of protein in the solution in units of micrograms (μg). Determine the quantity of protein in a solution that has an absorbance of 0.305. A blank solution has an absorbance of 0.060. The answer (Quantity of protein) should be in units of (μg)