?(a) Calculate the molarity of a solution made by dissolving 12.5 grams of \(\mathrm{Na}_{2} \mathrm{CrO}_{4}\) in enough water to form exactly 750 mL

Step 1 of 5) How many moles of KBr are present in 150 mL of a 0.112 M solutionHow many milliliters of 6.1 M HCl solution are needed to obtain 0.150 mol of HClIf a calorimetry experiment is carried out under a constant pressure, the heat transferred provides a direct measure of the enthalpy change of the reaction. Constant-volume calorimetry is carried out in a vessel of fixed volume called a bomb calorimeter. The heat transferred under constant-volume conditions is equal to ∆E. Corrections can be applied to ∆E values to yield ∆H.Because enthalpy is a state function, ∆H depends only on the initial and final states of the system. Thus, the enthalpy change of a process is the same whether the process is carried out in one step or in a series of steps. Hess’s law states that if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the steps. We can therefore calculate ∆H for any process, as long as we can write the process as a series of steps for which ∆H is known.