The enthalpies of formation of various iodine species are as follows: I(g), 107

Question

The enthalpies of formation of various iodine species are as follows: I(g), 107 kJ/mol; I2(g), 21 kJ/mol; HI(g), 26 kJ/mol. What other information is needed to calculate the enthalpy of the following reaction?

H2(g) + I2(g) = 2HI(g)

A the enthalpy of formation of gaseous iodine. B none, because the answer is 2x26 kJ. C the enthalpy of formation of gaseous hydrogen. D none, because the enthalpy of formation of an element in its stablest form is zero. E the enthalpy of formation of solid iodine. The enthalpies of formation of various iodine species are as follows: I(g), 107 kJ/mol; I2(g), 21 kJ/mol; HI(g), 26 kJ/mol. What other information is needed to calculate the enthalpy of the following reaction?

H2(g) + I2(g) = 2HI(g)

Explanation / Answer

option "D" is the right answer,because the enthalpies of stable forms are taken as zero....so h2 is a stable form in gaseous state......to caliculate enthalpy no further information needed

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