1. A 5.000 g sample of methanol, CH,OH, was combusted in the presenmce of excess oxygen in a bomb calorimeter containing 4000 g of water. The temperature of the water increased from 24.000 °C to 29.765 C. The heat capacity of the calorimeter was 2.657 kJC. The specific heat of water is 4.184 JigC Caleulate AE for the reaction in klmol.

A chemist measures the energy change AH during the following reaction: 2 Fe,O3(s) → 4 FeO(s)+O,(g) AH=560. kJ Use the information to answer the following questions. endothermic. This reaction is... х10 exothermic. Suppose 17.3 g of Fe,O, react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. kJ Round your answer to 3 significant digits.

An experiment is carried out where 12.2g of NaOH is dissolved in 240.0g of water in a coffee cup calorimeter. Dissolution is not a chemical reaction, but is a chemical process. NaOH(s) → Na+(aq) + OH-(aq) The mixture can be assumed to have the same specific heat capacity as liquid water  (4.18J/g.C) What is the massof the sorroundings where the temperature is being measured in this experiment?

E In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH), was added to 70.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 23.98 °C to 28.07 °C. If the solution has the same density and BO specific heat as water (1.00 g/mL and 4.184J/g °C,) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H₂O

8. A 1.107-g sample of benzoic acid (HC;H;O2) is burned in an excess of O:(g) in a bomb calorimeter, which is immersed in water. The reaction produces heat that causes the temperature of the water and bomb to increase from 24.96 to 29.20°C. (a) If the heat capacity of the calorimeter is 6.90 kJ/ºC, how many kilojoules of heat are produced by the combustion of 1.107 g of benzoic acid? (b) Calculate the heat of combustion per gram of benzoic acid and the molar enthalpy of combustion of benzoic acid.

You mix 125 mL of 0.230 M with 50.0 mL of 0.575 M in a coffee-cup calorimeter, and the temperature of both solutions rises from 22.30 °C before mixing to 24.96 °C after the reaction.   What is the enthalpy of reaction per mole of ? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g · K. Enthalpy of reaction =  ?

A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 26.8 ºC . What is qrxn in J?

A) When 1.911 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.410 °C to 26.630 °C. If the heat capacity of the calorimeter is 4.900 kJ/ °C, what is the heat of combustion of sucrose, in kJ/mol? And B) A 90.0 g piece of metal, initially at 98.60 °C, is placed into 120.0 g of water initially at 24.30 °C. If the final temperature of the water is 34.00 °C, what is the specific heat of the metal? (The specific heat of water is 4.184 J/g･ °C).

A 1.547 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and Its contains increases from 23.01C to 28.96C. The heat capacity (calorimeter constant) of the calorimeter is 41.65 kJ/C, what is the heat combustion per gram of the material? heat combustion

A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol