5.3 Enthalpy  (Page 10/25)

Explain how the heat measured in [link] differs from the enthalpy change for the exothermic reaction described by the following equation:
$\text{HCl}(aq)+\text{NaOH}(aq)⟶\text{NaCl}(aq)+{\text{H}}_2\text{O}(l)$

Using the data in the check your learning section of [link] , calculate Δ H in kJ/mol of AgNO ₃ ( aq ) for the reaction: $\text{NaCl}(aq)+{\text{AgNO}}_3(aq)⟶\text{AgCl}(s)+{\text{NaNO}}_3(aq)$

Calculate the enthalpy of solution (Δ H for the dissolution) per mole of NH ₄ NO ₃ under the conditions described in [link] .

Calculate Δ H for the reaction described by the equation. ( Hint : use the value for the approximate amount of heat absorbed by the reaction that you calculated in a previous exercise.)
$\text{Ba}{\left(\text{OH}\right)}_2\text{·}8{\text{H}}_2\text{O}(s)+2{\text{NH}}_4\text{SCN}(aq)⟶\text{Ba}{(\text{SCN})}_2(aq)+2{\text{NH}}_3(aq)+10{\text{H}}_2\text{O}\left(l\right)$

Calculate the enthalpy of solution (Δ H for the dissolution) per mole of CaCl ₂ .

Although the gas used in an oxyacetylene torch ( [link] ) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in [link] . Considering the conditions for which the tabulated data are reported, suggest an explanation.

How much heat is produced by burning 4.00 moles of acetylene under standard state conditions?

How much heat is produced by combustion of 125 g of methanol under standard state conditions?

How many moles of isooctane must be burned to produce 100 kJ of heat under standard state conditions?

What mass of carbon monoxide must be burned to produce 175 kJ of heat under standard state conditions?

When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?