Consider the reaction:Carried out at constant temperature and pressure. If ΔH and ΔU are enthalpy and internal energy changes for the reaction, which of the following expressions is true?a)ΔH = 0 b)ΔH = ΔU c)ΔH < ΔU d)ΔH > ΔUCorrect answer is option 'B'. Can you explain this answer?

Question

Consider the reaction:Carried out at constant temperature and pressure. If &#916;H and &#916;U are enthalpy and internal energy changes for the reaction, which of the following expressions is true?a)&#916;H = 0          b)&#916;H = &#916;U          c)&#916;H &#60; &#916;U       d)&#916;H &#62; &#916;UCorrect answer is option 'B'. Can you explain this answer?

Answer

When the process is isothermal change in temperature is zero so both delH and delU=0

Answer

∆H=∆U+∆nRT ∆n=-2
correct option is c
according to me

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