Using the equations N, (g) + O, (g)→ 2 NO (g) AH° = 180.6 kJ/mol N, (g) + 3 H, (g) → 2 NH, (g) AH° = -91.8 kJ/mol 2 H, (g) + O̟ (g)→ 2 H,Ó (g) AH° = -483.7 kJ/mol %3D Determine the enthalpy (in kJ/mol) for the reaction 4 NH, (g) + 5 O, (g) → 4 NO (g) + 6 H,0 (g).

The standard enthalpy change for the following reaction is 103 kJ at 298 K. N2(g) + O2(g) + Cl2(g) ---------> 2 NOCl(g)        ΔH° = 103  kJ What is the standard enthalpy change for this reaction at 298 K? 1/2 N2(g) + 1/2 O2(g) + 1/2 Cl2(g)-------->  NOCl(g)  kJ

A 837837 g copper pan is removed from the stove at a temperature of 150 °C. It is then stacked on top of a 787787 g aluminum sheet at room temperature, 25 °C. The specific heat capacity for copper is 0.387 Jg·KJg·K and that for aluminum is 0.904 Jg·KJg·K. Assume no heat is gained or lost to the surroundings.   What is the final temperature (?fTf) of the two objects after thermal equilibrium is reached?

Consider the following reaction: 2 CH3OH(g)  →  2 CH4(g)  +  O2(g)      ΔH = +252.8 kJ Is this reaction exothermic or endothermic? Endothermic   Calculate the amount of heat transferred when 24.0g of CH3OH is decomposed by this reaction at constant pressure.

When 200.0 mL of 0.862 M HCI is mixed with 200.0 mL of 0.431 M Ba(OH)2 in a coffee cup calorimeter, the temperature of the solution increases from 21.35°C to 27.05°C. Given the specific heat of solution of 4.18 J g1 °C-l and assuming the density of each solution to be 1.00 g/mL, what is the heat of reaction in kJ per mole of HCl? The neutralization reaction is: 2 HCI(aq) + Ba(0H)2(aq) → BaCl2(aq) + 2 H20(1) Select one: -55.3 kJ/mol HCI -9.53 kJ/mol HCI O - 110.6 kJ/mol HCI O 110.6 kJ/mol HCl 55.3 kJ/mol HCI O 9.53 kJ/mol HCI ВАCK Question 5 of 6 NEXT étv A

What is the AH°rxn for the reaction of gaseous ammonia and oxygen gas to form gaseous nitrogen monoxide and water vapor? Use the given standard heats of formation. Write the balanced chemical reaction. AH°; NH3 (g) AH°;02 (g) = 0 AH°;NO (g) = 103.56 kJ/mol AH°; H20 (g) = -218.42 kJ/mol = -38.17 kJ/mol %3D

Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g)- →C4H₁0(g) ΔΗ° = -125.6 kJ (2) C₂H4(g)- →2C(s) + 2H₂(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C₂H4(g) + H₂(g) →C4H10(g) kj AH° = ?

The enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/mol

56

Calcium carbonate can be decomposed upon applying heat with the following equation CaCO3(s)  →  CaO(s)  +  CO2(g)    ΔH = +179.5kJ How much heat will be needed to decompose 30 g of calcium carbonate?  AND What size container will be required (in L) to contain the carbon dioxide generated at 25ºC and 1.2 atm?