3. Consider the following two reactions:                         A → 2B           ΔH0rxn = 456.7 kJ/mol                         A → C ΔH0rxn = -22.1kJ/mol Determine the enthalpy change for the process for 2B → C.

In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 24.0°C. After the reaction, 3 the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ - kJ/mol

A bomb calorimeter has a heat capacity of 2.47 kJ/?. When a 1.00 mol sample of a certain hydrocarbon was burned in this calorimeter, the temperature increased by 2.14?. Calculate the heat of combustion per mole of the hydrocarbon.

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 =  ?

Calcium hydroxide is prepared by adding calcium oxide to water: CaO (s) + H2O (l) → Ca(OH)2 (s) Calculate the enthalpy change (ΔH) for this reaction considering the following experiment.  A 10.0 g sample of CaO (s) {MM = 56.08 g/mol} is added to 1.00 liter of water in a calorimeter with a total heat capacity of 4.37 kJ K-1 and the temperature increases by 2.70 K.

In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ = 0.182 kJ/mol

In the following experiment, a coffee-cup calorimeter containing 100 g of H20 is used. The initial temperature of the calorimeter is 23.0 °C. If 4 g of CaClzis added to the calorimeter, what will be the final temperature of the solution in the calorimeter? Assume that the heat capacity of the solution is 4.18 J/g°C, and that the heat capacity of the calorimeter is negligible. The heat of dissolution AHsolin of CaCl2 is -82.8 kJ/mol. Enter your answer numerically in terms of °C.

A chemist measures the energy change AH during the following reaction: 2 NH3(g) → N₂(g) +3H₂(g) Use the information to answer the following questions. This reaction is... ΔΗ= 160. kJ Suppose 15.4 g of NH3 react. Will any heat be released or absorbed? 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. Be sure your answer has the correct number of significant digits. endothermic. exothermic. Yes, absorbed. Yes, released. No. ПkJ x10 X Ś

Titanium reacts with iodine to form titanium(III) iodide, emitting heat:2 Ti(s) + 3 I2(g) ---------> 2 TiI3(s) ∆H°rxn = -839 kJDetermine the masses of titanium and iodine that react if 1.55 x 103 kJ of heat is emitted by the reaction.

When CO(g) reacts with NO(g) according to the following reaction, 373 kJ of energy are evolved for each mole of CO(g) that reacts. Complete the following thermochemical equation. 2CO(g) + 2NO(g)- →2CO₂(g) + N₂(g) ΔΗ = kJ