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Chapter 10: Problem 4
The equations showing the effect of temperature change on the heat of reaction is known as (a) Arrhenius equation (b) Kirchhoff's equation (c) Ostwald's equation (d) none of these
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"The resultant heat change in a chemical reaction is the same whether it takes place in one or several stages." This statement is called (a) Le-Chatelier's principle (b) Hess's law (c) Lavoisier-Laplace law (d) Joule-Thomson effect
Standard heat of formation of an element is (a) infinite (b) zero (c) \(100 \mathrm{~kJ}\) (d) \(200 \mathrm{~kJ}\)
The enthalpies of elements in their standard states are taken as zero. Thus, the enthalpy of formation of a compound (a) will always be positive (b) will always be negative (c) may be positive or negative (d) will always be zero
Endothermic reaction is one in which (a) heat is converted into electricity (b) heat is absorbed (c) heat is given out (d) heat is converted into mechanical work
A reaction whose heat of reaction shows the bond energy of \(\mathrm{HCl}\) is (a) \(\mathrm{HCl}(\mathrm{g}) \longrightarrow \mathrm{H}(\mathrm{g})+\mathrm{Cl}(\mathrm{g})\) (b) \(2 \mathrm{HCl}(\mathrm{g}) \longrightarrow \mathrm{Hl}(\mathrm{g})+\mathrm{Cll}(\mathrm{g})\) (c) \(\mathrm{HCl}(\mathrm{g}) \longrightarrow \frac{1}{2} \mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{Cl}_{2}(\mathrm{~g})\) (d) \(\mathrm{HCl}(\mathrm{g}) \longrightarrow \mathrm{H}^{+}(\mathrm{g}) \longrightarrow \mathrm{Cl}^{-}(\mathrm{g})\)
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