List of top Chemistry Questions asked in Assam CEE

For the following reaction at 298 K: \[ \text{30O}_2(g) \rightleftharpoons \text{20O}_3(g) \quad \Delta H = +285 \, \text{kJ/mol} \] The equilibrium constant, \( K_c \), is \[ K_c = 2.47 \times 10^{-31} \quad \text{at 298 K. The value of \( K_c \) will increase when} 298 \, \text{K is} \quad \text{increased.} \]

For the reaction, \( A + B \rightarrow \) products, the following data is obtained: A + B \( \rightarrow \) products, the following data is given: $$ \begin{array}{|c|c|c|c|} \hline \text{Exp. No.} & [A] \, (\text{mol L}^{-1}) & [B] \, (\text{mol L}^{-1}) & \text{Initial rate} \, (\text{mol L}^{-1} s^{-1}) \\ \hline 1 & 0.2 & 0.4 & 0.8 \\ 2 & 0.4 & 0.2 & 1.6 \\ 3 & 0.3 & 0.2 & 0.4 \\ \hline \end{array} $$ The rate law of the reaction is: 

For the following reaction \[ 2 \text{Mn}^{3+} (\text{aq}) + 3 \text{N}_2^{2+} (\text{aq}) \rightarrow 3 \text{Mn}^{2+} (\text{aq}) + 2 \text{N}_2 (\text{s}) \] The standard Gibbs free energy change (\(\Delta G^\circ\)) of the reaction is

The standard electrode potential of electrode-A and electrode-B are \(-0.25 \, \text{V}\) and \(-0.76 \, \text{V}\), respectively. If a Galvanic cell is created using these two electrodes, the standard electromotive force (EMF) of this cell will be:

The main product formed in the following reaction is: \[ CH_3 - CH_2 - CH = CH_2 + HBr \longrightarrow \]