The relationship between Young's modulus ($Y$), stress ($\sigma$), and strain ($\epsilon$) is given by:
\[ Y = \frac{\sigma}{\epsilon} \]
We need to find the limiting stress ($\sigma$). Rearranging the formula, we get: \[ \sigma = Y \times \epsilon \] Substituting the given values:
\[ \sigma = (2 \times 10^{11} \, \text{N/m}^2) \times (0.15) \] \[ \sigma = 0.30 \times 10^{11} \, \text{N/m}^2 \] \[ \sigma = 3.0 \times 10^{-1} \times 10^{11} \, \text{N/m}^2 \] \[ \sigma = 3.0 \times 10^{(-1 + 11)} \, \text{N/m}^2 \] \[ \sigma = 3.0 \times 10^{10} \, \text{N/m}^2 \] The value of limiting stress is \(3 \times 10^{10} \, \text{N/m}^2\).
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.