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.

Answer 1

To calculate the final temperature of the solution, you need to use the equation q = mcΔT. Calculate the heat released by the reaction using the equation q = -ΔH. Calculate the moles of BE(NO3)2 and NaF, and use the molar ratio to find the moles of NaF. Use the equation q = mcΔT to calculate the final temperature of the solution.

Step-by-step explanation:

The final temperature of the solution can be determined using the equation q = mcΔT, where q is the heat absorbed or released, m is the mass of the solution, c is the specific heat capacity of the solution, and ΔT is the change in temperature. In this case, the reaction is exothermic, so heat is released. First, calculate the heat released by the reaction using the equation q = -ΔH, where ΔH is the enthalpy change. Since the reaction goes to completion, the moles of BE(NO3)2 will be equal to moles of NaF. Calculate the moles of BE(NO3)2 using the equation M = moles/L, where M is the molarity and L is the volume in liters.

Then, use the molar ratio from the balanced equation to calculate the moles of NaF. Multiply the number of moles by the molar mass of NaF to find the mass. Now, use the equation q = mcΔT to calculate the heat released or absorbed by the solution. Substitute the values into the equation and solve for ΔT.