Consider the reaction. 2 Fe, O3 → 4 Fe + 30, AHn = +824.2 kJ rxn The formation of 88.0 g of Fe results in the release of 1.30 × 10' kJ of heat. the absorption of 1.30 × 10' kJ of heat. the absorption of 325 kJ of heat. the release of 325 kJ of heat. the absorption of 18100 kJ of heat. the release of 18100 kJ of heat.

22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.

Consider the reaction.   2Fe2O3⟶4Fe+3O2        Δ?∘rxn=+824.2 kJ   The decomposition of 74.0 g of Fe2O3 results in A.) the release of 382 kJ of heat. B.) the absorption of 191 kJ of heat. C.) the release of 191 kJ of heat. D.) the absorption of 30500 kJ of heat. E.) the release of 30500 kJ of heat. F.) the absorption of 382 kJ of heat.

The reaction below is a  exothermic or endothermic reaction. 2SO3(g) + Heat ⇋ 2SO2(g) + O2(g)

A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?

3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g °C and the density of the water is 1.00 g/ mL). You can assume that the specific heat of the solution is the same as that of water.

15. The enthalpy change for the reaction CH,(g) + 20,(g) CO,(g) + 2H,O() is -891 kJ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?

In a coffee cup calorimeter with a heat capacity of 21.5 J/ºC, 225 mL of 0.20 M KOH at 22.3 ºC neutralizes 225 mL of 0.20 M HCl at 22.3 ºC. After the reaction occurs, the temperature of the resulting mixture is 29.2 ºC. The density of the final solution is 1.00 g/mL and the specific heat is 4.18 J/g°C. Calculate the Heat of neutralization of KOH.

When a 0.740-g sample of trinitrotoluene (TNT), C,H,N,O, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter and its content is 3.35 kJ/°C. How much heat was produced by the combustion of the TNT sample? O 34.2 kJ O 11.7 kJ O 101.5 kJ

Consider the reaction. 2 Fe,O, 4 Fe + 30, AHn = +824.2 kJ The formation of 84.0 g of Fe results in the absorption of 3.10 x 102 kJ of heat. the absorption of 17300 kJ heat. the absorption of 1240 kJ of heat. the release of 1240 kJ of heat. the release of 3.10 x 10² kJ of heat. the release of 17300 kJ of heat. G Search or type URL