Experiment 14 Data and Calculations: Heat Effects and Calorimetry A. Specific Heat Trial 1 Trial 2 Mass of stoppered test tube plus metal Mass of test tube and stopper Mass of calorimeter g Mass of calorimeter and water 59.69 9,50 71435 ge Mass of water g Z0 44 6S.24 65.29 gg Mass of metal 2122C Initial temperature of water in caiemeter Initial temperature of al ne i0C unless directed to do ewiech 100 °C ° C Equilibrium temperature of metal and water 79.3 "C ОС in calorimeter °C ° C ALwater (Ffinal-Finitial) °C ° C Afmetal J J Яно J/g C J/g°C Specific heat of the metal (Eq. 3) Approximate molar mass of metal HLO Unknown metal # 146.643 B. Heat of Solution Mass of calorimeter plus water 65.7113 Mass of beaker (continued on following page)

If the following three thermochemical equations are added together, what is the resulting equation:2 XO2 (g) +2 CO (g) →→ 2 XO (g) + 2 CO2 (g)2 XO (g) + 2/3 CO2(g) →→ 2/3 X3O4 (s) + 2/3 CO (g)2/3 X3O4 (s) + 1/3 CO2 (g) →→ X2O3 (g) + 1/3 CO (g)     Question 17 options:   6 XO (g) + 2 CO2(g) →→ 2 X3O4 (s) + 2 CO (g)   2 XO2 (s) + CO (g) →→ X2O3 (s) + CO2 (g)   C (s) + 3 XO2 (g) →→ X3O4 (g) + CO2 (g)   2 X3O4 (s) + CO2 (g)  →→ 3 X2O3 (g) + CO (g)   CO (g) + XO2 (g) →→ XO (g) + CO2 (g)

Use the given equations to determine the enthalpy, ΔHrxn, per mole of reaction for the chemical equation below. Report your answer to one decimal place and do not include units.  P4(s) + 6H2(g) + 6O2(g) → 4H3PO3(aq)

What amount of heat in Joules is required to raise the temperature 0f 10.0g of aluminum by 15.0 Celsius degrees?

6) A block of rhenium metal (specific heat =0.0329 cal/ gC) is heated to 88.2C and then dropped into 100.0 g of water initially at 26.4 C. The final temperature of the mixture is 32.4C. What was the mass of the block of rhenium?

29. (a) (b) (c) What is the definition of the specific heat of water? the amount of heat required to melt one mole of a substance at the melting point. the amount of heat required to vaporize one mole of a Kryptonite at the boiling point. the amount of heat required to raise the temperature of 1 gram of water by 1°C.

Please don't provide handwritten solution.....

How much heat is given off to the surroundings when 6 g of aluminum reacts according to the following equation? Express your answer correctly rounded to two decimal places.2 Al + Fe2O3  Al2O3 + 2 Fe ΔH°rxn = -849 kJ. kJIf all of the heat generated by the reaction was absorbed by one liter of room temperature water, what would be the highest temperature the water could reach? Express your answer correctly rounded to two decimal places. °CWhile writing this question, I had to take into account that the final temperature reachable in the previous question could not exceed the boiling point of water. Given this information, what is the highest whole number amount of aluminum that could have been used for this question? Enter only a number for your answer. g