Question

When 50.0ml of 0.300 m be(no3)2 is added to 50.0ml of 0.800 m naf the salt bef2 precipitates, as shown in the net ionic equation below, the initial temperrature of both soclutions is 20.0 degrees c. assuming the reaction goes to completion, that the solution is well insulated from the surruondings and that the resulting solution has a density of 1.00g/ml and a specific heat of 4.184k/g degrees c, calculate the final temperature of the solution. the delta h value is -120 kj.

Be2+(aq) + 2 F-(aq) → BeF2(s)∆H°=-11.5 kJ

Answer 1

To calculate the final temperature after mixing Be(NO3)2 and NaF, the heat released or absorbed calculated using the provided enthalpy change and the specific heat equation would be necessary along with further details on the reaction's stoichiometry and the mass of the resulting solution.

Step-by-step explanation:

When 50.0 mL of 0.300 M Be(NO3)2 is mixed with 50.0 mL of 0.800 M NaF, BeF2 precipitates, with a given enthalpy change (ΔH) of -11.5 kJ for the reaction.

As the specific heat is given as 4.184 J/g degrees Celsius and the density of the resulting solution is 1.00 g/mL, we can calculate the final temperature of the solution after the reaction goes to completion. Given the data, assume the solution behaves similarly to water in terms of its thermodynamic properties.

To solve for the final temperature, you would calculate the amount of heat released or absorbed using the given enthalpy change, and apply this to the specific heat equation q = mcΔT, where q is heat transfer, m is mass, c is specific heat, and ΔT is change in temperature.

However, the necessary calculations are not provided here due to insufficient information on the reaction's stoichiometry and lack of the mass of the final solution that would be needed for a complete calculation.