Thermochemical Equations
Chemistry ⇒ Thermochemistry and Energetics
Thermochemical Equations starts at 10 and continues till grade 12.
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Describe how to write a thermochemical equation for the dissolution of NaCl(s) in water, given \Delta H = +3.9\ \mathrm{kJ}/\mathrm{mol} .
Describe the difference between an endothermic and an exothermic thermochemical equation.
Describe the steps to write a thermochemical equation for the neutralization of HCl(aq) with NaOH(aq), given \Delta H = -57.1\ \mathrm{kJ}/\mathrm{mol} .
Explain why it is important to specify the physical states of substances in a thermochemical equation.
Explain why the enthalpy change for a reaction is an extensive property.
Explain why the enthalpy change for the vaporization of water is different from that for the fusion of ice.
Given the following thermochemical equations: (1) \mathrm{C}(s) + \mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g);\ \Delta H = -393.5\ \mathrm{kJ} , (2) \mathrm{H}_{2}(g) + \frac{1}{2}\mathrm{O}_{2}(g) \rightarrow \mathrm{H}_{2}\mathrm{O}(l);\ \Delta H = -285.8\ \mathrm{kJ} , calculate the enthalpy change for the reaction: \mathrm{C}(s) + 2\mathrm{H}_{2}(g) + \mathrm{O}_{2}(g) \rightarrow \mathrm{CH}_{3}\mathrm{OH}(l) , given \Delta H_{f}^{\circ} (\mathrm{CH}_{3}\mathrm{OH}) = -238.7\ \mathrm{kJ} .
Given the thermochemical equation: 2\mathrm{Al}(s) + 3\mathrm{Cl}_{2}(g) \rightarrow 2\mathrm{AlCl}_{3}(s) ; \Delta H = -1408\ \mathrm{kJ} , what is the enthalpy change for the formation of 1 mole of \mathrm{AlCl}_{3}(s) ?
Given the thermochemical equation: 2\mathrm{H}_{2}\mathrm{O}_{2}(l) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{O}_{2}(g) ; \Delta H = -196\ \mathrm{kJ} , what is the enthalpy change for the decomposition of 1 mole of \mathrm{H}_{2}\mathrm{O}_{2}(l) ?
Given the thermochemical equation: 2\mathrm{SO}_{2}(g) + \mathrm{O}_{2}(g) \rightarrow 2\mathrm{SO}_{3}(g) ; \Delta H = -198\ \mathrm{kJ} , what is the enthalpy change for the production of 4 moles of \mathrm{SO}_{3}(g) ?
Given the thermochemical equation: \mathrm{CaCO}_{3}(s) \rightarrow \mathrm{CaO}(s) + \mathrm{CO}_{2}(g) ; \Delta H = +178\ \mathrm{kJ} , is the reaction endothermic or exothermic?
Given the thermochemical equation: \mathrm{N}_{2}(g) + 3\mathrm{H}_{2}(g) \rightarrow 2\mathrm{NH}_{3}(g) ; \Delta H = -92\ \mathrm{kJ} , what is the enthalpy change for the formation of 1 mole of \mathrm{NH}_{3}(g) ?
If the enthalpy change for a reaction is written as ΔH = -200 kJ, what does the negative sign indicate?
If the thermochemical equation for the formation of water is: 2\mathrm{H}_{2}(g) + \mathrm{O}_{2}(g) \rightarrow 2\mathrm{H}_{2}\mathrm{O}(l);\ \Delta H = -572\ \mathrm{kJ} , what is the enthalpy change for the formation of 1 mole of water?
What is a thermochemical equation?
Write the thermochemical equation for the combustion of methane ( \mathrm{CH}_{4} ) in oxygen, given that \Delta H = -890\ \mathrm{kJ}/\mathrm{mol} .
