Question

Fill in the Blanks Let's use calorimetry to measure heats of reaction. Suppose you mix 25.0 mL of 0.08M cesium hydroxide with 25.0 mL of 0.08M hydrochloric acid. Assume both solutions are at 28.0°C. The temperature of the solution after the reaction is 30.2°C. Because the temperature of the solution went up, the reaction is (endothermic/exothermic). Now compute the heat of the reaction assuming the heat capacities of the solutions are equal to pure water (4.18 J/g°C). Report the Q as positive if you thought the reaction was endothermic and negative if you thought it was exothermic. The Qis Joules. The heat of the reaction is generally reported as heat per mole. The moles of acid = moles of base in this case and these moles are Therefore the heat of the reaction (in kJ/mole) is [] Full

Answer 1

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- The temperature of solution is * Therefore heat is released from the reaction rising- Hence exothermic" Milli moles of CSOH = Molarity x Vol (me E 0-08 M X 25 ml E 2 MM. Millimoles of Hee = 0.08 M x 25 ml = 9mm सिक weight of solb = B. weight of CSOM I t weight of He 150 x 9x10-3 + 36-5x2x10-3 = = 0.313 g 0= m Cp PT = 0·373 x 4.18 (32-2-28) = -6:55 J (: exothermic) moles of acid: moles of base = 2x10 mole (as calculated above) -6.55 388 - 3.275 kJ/mol 1000 X 2 X10-3 Heat (KJ/mol) =