Enthalpy of combustion of carbon to carbon dioxide is \(-390.0~\text{kJ mol}^{-1}.\) The amount of heat released when \(35.0~\text{g}\) of \(\mathrm{CO_2}\) is formed from the reaction of carbon and dioxygen gas, is:
What is the correct relationship between changes in enthalpy and internal energy within the following options?
1. \(\Delta \mathrm{H}+\Delta \mathrm{U}=\Delta \mathrm{nR} \)
2. \(\Delta \mathrm{H}=\Delta \mathrm{U -\Delta n_gRT}\)
3. \(\Delta \mathrm{H}=\Delta \mathrm{U+\Delta n_gRT }\)
4. \(\Delta \mathrm{H} -\Delta \mathrm{U=-\Delta n_gRT}\)
Subtopic: Enthalpy & Internal energy |
80%
From NCERT
NEET - 2023
Other Reason
Add Note
Please attempt this question first.
Hints
Please attempt this question first.
Upgrade Your Plan
Upgrade now and unlock your full question bank experience with daily practice.