The given expression is \( (666 \ldots \text{up to } n \text{ digits})^2 + (888 \ldots \text{up to } n \text{ digits}) \).
We know that \( 666 \ldots \) up to \( n \) digits is represented as \( \frac{2}{3}(10^n - 1) \) and \( 888 \ldots \) up to \( n \) digits is represented as \( \frac{8}{9}(10^n - 1) \). Now, square \( 666 \ldots \): \[ \left( \frac{2}{3}(10^n - 1) \right)^2 = \frac{4}{9}(10^{2n} - 2 \times 10^n + 1). \] And for \( 888 \ldots \), we have: \[ \frac{8}{9}(10^n - 1). \] Adding both, the final result is: \[ \frac{4}{9}(10^{2n} - 1). \]
At 15 atm pressure, $ \text{NH}_3(g) $ is being heated in a closed container from 27°C to 347°C and as a result, it partially dissociates following the equation: $ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) $ If the volume of the container remains constant and pressure increases to 50 atm, then calculate the percentage dissociation of $ \text{NH}_3(g) $
If equilibrium constant for the equation $ A_2 + B_2 \rightleftharpoons 2AB \quad \text{is} \, K_p, $ then find the equilibrium constant for the equation $ AB \rightleftharpoons \frac{1}{2} A_2 + \frac{1}{2} B_2. $
Consider the following reaction: $ \text{CO}(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) $ At 27°C, the standard entropy change of the process becomes -0.094 kJ/mol·K. Moreover, standard free energies for the formation of $ \text{CO}_2(g) $ and $ \text{CO}(g) $ are -394.4 and -137.2 kJ/mol, respectively. Predict the nature of the above chemical reaction.