\(2HC = CH_2\text{Cl}_2 \xrightarrow{\text{A}} \text{NH}_4\text{Cl}\) \(\xrightarrow{\text{B}}\) \(\text{Identify the compounds A and B}\)
Consider the following reactions, C(s) + O2(g) → CO2(g), \(\Delta\) H = -94\(\text{ kcal}\) 2CO(g) + O2 → 2CO2(g), \(\Delta\) H = -135.2\(\text{ kcal}\) Then, the heat of formation of CO (g) is:
\(NH_3\) molecule attract \(H^+\) ion towards itself to form ammonium ion \({NH}_4^+\) through:
In the redox reaction \[ \text{MnO}_4^- + \text{C}_2\text{O}_4^{2-} \to \text{Mn}^{2+} + \text{CO}_2 + \text{H}_2\text{O} \] The correct coefficients of \( \text{C}_2\text{O}_4^{2-} \) and \( \text{H}^+ \) are
For the reactions \(C + O2 \rightarrow CO2\); \(\, \Delta H = -393 \, \text{kJ} 2Zn + O2 \rightarrow 2ZnO\), \(\, \Delta H = -412 \, \text{kJ}\) \(\text{the correct statement is:}\)
A cell has been set up as shown in the following diagram and E$^0$ has been measured as 1.00V at 25°C. Calculate $\Delta$G$^0$ for the reaction.
