04 A student mixed 25.0 ml of 1.50 M HCl and 25.0 ml of 1.50 M NaOH, both at 22.50 °C, in a coffee cup calorimeter. The

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04 A Student Mixed 25 0 Ml Of 1 50 M Hcl And 25 0 Ml Of 1 50 M Naoh Both At 22 50 C In A Coffee Cup Calorimeter The 1 (29.46 KiB) Viewed 148 times

04 A student mixed 25.0 ml of 1.50 M HCl and 25.0 ml of 1.50 M NaOH, both at 22.50 °C, in a coffee cup calorimeter. The temperature of the mixture rose to 32.70 °C Assume that the density of the resulting solution is 1.0 g/mL and the specific heat of the solution is 4.181/8*0, (A) Write a balanced chemical equation for the reaction (B) Calculate the amount of heat absorbed by the resulting solution (C) How much heat is released by the reaction? (D) Calculate oH for the reaction per mole of the base Q5. Using the values from the Appendix in your text, calculate the enthalpy of reaction as for the following reactions: 2. NO.(e) +4 Hz N. e)+4 H0 () b. 3 NO:(8)+HOM) → 2 HNO3(aq) + NO(g) C.0,(s) + 3 CO(s) → 2 Cr(s) + 3 CO2(6)