(b) A sample of Magnesium metal weighing 0.14g is combusted in a bomb calorimeter containing 3.0 x 10°g water at an initial temperature of 25°C. The maximum temperature recorded was 26°C. If the heat capacity of the calorimeter is 1769J °C' and the specific heat of water is 4.184 Jg1 °C'. Calculate the enthalpy of combustion of Magnesium

A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g•°C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.

A 110.2 mL sample of 1.00 M NaOH is mixed with 55.1  mL of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.85 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 31.30 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g·°C), and that no heat is lost to the surroundings.   a. Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation.   b. Is any NaOH or H2SO4 left in the Styrofoam cup when the reaction is over?A.   No B.   Yes  c. Calculate the enthalpy change per mole of H2SO4 in the reaction.     kJ/mol

In this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, delta Hdiss or rxn.  A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the total mass of the solution in sig figs?    mass  = 4.368 g + 35.5 g = 39.868 g   a. 39.8 g b. 40 g c. 39 g d. 39.868 g e. 4.0 x 10^1 g f. 39.87 g g. 39.86 g h. 39.9 g i. none of these

(b) What is the specific enthalpy of combustion of ethane? kJ/g. 3 sig. number.

The enthalpy of combustion of benzoic acid (C,H,COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has P mol been accurately determined to be -3226.7 - When 2.5311 g of benzoic acid are burned in a calorimeter, the temperature rises from 20.84 °C to 26.67 °C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g) Round your answer to 3 significant digits. Note: Reference the Phase change properties of pure substances table for additional information. 0-/2 0.8 X 5 8 @ al P

The standard heat of formation, AH;, is defined as the enthalpy change for the formation of one mole of Part B substance from its constituent elements in their standard states. Thus, elements in their standard states have AH: = 0. Heat of formation values can be used The combustion of ethene, C2H4, occurs via the reaction to calculate the enthalpy change of any reaction. C2H4 (g) + 302 (g)→2CO2(g) + 2H20(g) Consider, for example, the reaction with heat of formation values given by the following table: 2NΟ (5) + Ο, (s) 2ΝO, (g) ΔΗρ (kJ/mol) Substance with heat of formation values given by the following table: C2H4 (g) 52.47 CO2 (g) -393.5 Substance (kJ/mol) H2O(g) -241.8 NO(g) 90.2 Calculate the enthalpy for the combustion of ethene. 02 (g) Express your answer to four significant figures and include the appropriate units. NO2(g) 33.2 • View Available Hint(s) Then the heat of formation for the overall reaction is ΔΗ ΔΗ (products) -ΔΗ; (reactants ) [2(90.2) + 0] HA ? 2(33.2) -114 kJ/mol…