Given the following thermochemical equations (in the picture), 1. Calculate the value of Ho (in kilojoules) for the reaction: 1/2 Cl2 (g) + NaBr (s) ----> NaCl (s) + 1/2 Br2 (l) b. Is the reaction exothermic or endothermic?

When the Cacl2(s) is added to water, the following reaction occurs. Cacl (s) – Ca²"(aq) + 2CI"(aq) AH = - 81.5 kJ A 24.1 g sample of Caclz is dissolved in water, with both substances at 25.0 °C. Calculate the final temperature (in °C) of the solution assuming no heat is lost to the surroundings, the final solution, containing Cacl2 and water, has a mass of 100.0 g and the solution has a specific heat capacity of 4.18 J °c-lg-1. The molar mass of CaCl2 = 110.98 g/mol Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to one (1) decimal place. Answer: 59.0 The correct answer is: 67.3

Find the enthapy change for the reaction below in kJ .                   4NH3(g)  + 5O2(g) --> 4NO(g) + 6H2O(g)     ΔH= ?    Given :  (NH3(g)) = -46.1,         (NO(g)) =  + 90.3 kJ/mol   and        (H2O(g)) = -241.8 kJ/mol.

Given: 4AICI3(s) + 302(g) → 2Al,O3(s) + 6C12(g); AH=-529.0 kJ determine AH for the following thermochemical equation. Cl,(3) + Al,O;(s) → AICI,(9) + 02(g) O +88.2 kJ O +264.5 kJ O +176.3 kJ O -176.3 kJ O +529.0 kJ

4. Consider the equations for these reactions: % N2 + % O2 → NO NO2 → NO + % 02 AH = +90.4 kJ AH = +56.5 All reactants are gaseous. What is the heat of formation (AH;) for NO2 gas?

The combustion of a sample of isoctane vapor at constant pressure raises the temperature of a calorimeter and its contents by 0.400 °C. The heat capacity of the calorimeter and water combined is 2.48 kJ/°C. How much heat was produced from the combustion? (variations of formula: c=q/mat)

Consider an endothermic reaction that takes place in 303 mL of solution.  If the reaction requires 4,468 J of energy and the initial temperature of the solution is 26.7, what will the final solution temperature be? (3 sf) The density of solution is 1.00 g/mL and the specific heat of the solution is the same as that of water.

Octane (C8H18) is a component of gasoline that burns according to the following equation:  C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?

a) Given that AgNO3 is -124.4 kJ/mol, at standard conditions, what is dH when 56g of AgNO3 (M = 169.9 g/mol) reacts?   b) If the heat involved (derived from answer a) is transferred without loss to 100.0g of water at 25ºC, what is the final temperature of the water (CH2O = 4.18J/gºC)?

How much heat is evolved when 8.89x10° g of ammonia is produced according to the following equation? (Assume that the reaction occurs at constant pressure.) N2(9) + 3H,(g) - 2NH3(g); AH = -91.8 k) kJ evolved