Answered

Find the best answers to your questions with the help of IDNLearn.com's expert contributors. Ask your questions and receive reliable, detailed answers from our dedicated community of experts.

Generic solid, X, has a molar mass of 64.6 g/mol. In a constant-pressure calorimeter, 37.8 of X is dissolved in 263 g of water at 23.00 °C.X(s) — X(aq) The temperature of the resulting solution rises to 24.40 °C. Assume the solution has the same specific heat as water, 4,184 J/(g ⋅ °C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = _________ kJ What is the enthalpy of the reaction? DeltaH rxn = ____________ kJ/mol

Sagot :

In order to find letter A, we need to calculate all this information using this calorimetry formula:

Q = mcΔT

Where:

Q = heat absorbed or released

m = mass

c = specific heat

ΔT = variation in temperature

Now placing the values of our question in the formula:

Q = 263g * (4.184J/g°C) * (24.40 - 23)

Q = 1540.54J

Q = 1.54 kJ

Now in letter B we need to use the

ΔH = Q/n

Where:

ΔH = enthalpy of the reaction

Q = the heat

n = number of moles

We need to find the number of moles first, we know that the molar mass is 64.6g/mol and we have 37.8g, therefore:

64.6g = 1 mol

37.8g = x moles

x = 0.58 moles of X

Now our equation:

ΔH = 1.54/0.58 moles

ΔH = 2.65 kJ/mol

Thank you for using this platform to share and learn. Keep asking and answering. We appreciate every contribution you make. For dependable and accurate answers, visit IDNLearn.com. Thanks for visiting, and see you next time for more helpful information.