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Fifty (50.0) mL of 1.25 M AgNO3 and 50.0 mL of 1.75 M HCl are mixed...

Fifty (50.0) mL of 1.25 M AgNO3 and 50.0 mL of 1.75 M HCl are mixed in a coffee cup calorimeter resulting to a mass of solution equal to 101 g. If the two solutions are initially at 25.40 °C and the final T is 22.30 °C. Assume that the specific heat of solution is equal to that of water (4.18 J/g oC). What is the theoretical yield (mol AgCl) & What is the qreaction in kJ/mol AgCl?

Is the ANSWER D?????

A . 0.088 mol AgCl & 15 kJ/mol AgCl

B. 0.088 mol AgCl & 21 kJ/mol AgCl

C. 0.063 mol AgCl & 15 kJ/mol AgCl

D. 0.063 mol AgCl & 21 kJ/molAgCl

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Answer #1

The correct option is (D).

Reaction: AgNO3 (aq) + HCl (ar) → AgNO₃ Car + hoe Age(s) + HNO₃ caq, Moles of He = volume in Lx Molarity in mol/l = (50) L xGiven mass of solution = 1019 Now, a, -mco 1. Von = -mcat --1019 x 4.18 5 x (2230-25-40)°C goc = 1308.758 J V xn in kJ/mol Ag

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