We are given a triangle \( ABC \) where the angles \( A \), \( B \), and \( C \) are in A.P. This implies:
\[ A - B = B - C \quad \Rightarrow \quad 2B = A + C. \] Therefore, \[ B = \frac{A + C}{2}. \] Next, we need to find the expression for \( \frac{a + c}{b} \), where \( a \), \( b \), and \( c \) are the sides opposite to angles \( A \), \( B \), and \( C \), respectively.
Step 1: Use the Law of Sines.
By the Law of Sines, we know: \[ \frac{a}{\sin A} = \frac{b}{\sin B} = \frac{c}{\sin C}. \] From this, we can express the sides in terms of the sine of the angles: \[ a = k \sin A, \quad b = k \sin B, \quad c = k \sin C, \] where \( k \) is the common constant, \( \frac{a}{\sin A} = \frac{b}{\sin B} = \frac{c}{\sin C} \).
Step 2: Expression for \( \frac{a + c}{b} \).
We need to find: \[ \frac{a + c}{b} = \frac{k (\sin A + \sin C)}{k \sin B}. \] Simplifying: \[ \frac{a + c}{b} = \frac{\sin A + \sin C}{\sin B}. \] Using the sum of sines identity: \[ \sin A + \sin C = 2 \sin \left( \frac{A + C}{2} \right) \cos \left( \frac{A - C}{2} \right). \] Therefore, the expression becomes: \[ \frac{a + c}{b} = \frac{2 \sin \left( \frac{A + C}{2} \right) \cos \left( \frac{A - C}{2} \right)}{\sin B}. \] Since \( B = \frac{A + C}{2} \), we have: \[ \frac{a + c}{b} = 2 \cos \left( \frac{A - C}{2} \right). \] Thus, the correct answer is \( B \).



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.