We are given the following two equations:
1. \( f(x) + g(x) = e^x \) 2. \( f(x) - g(x) = e^{-x} \)
Step 1: Add the two equations.
By adding the two
given equations, we get:
\[ (f(x) + g(x)) + (f(x) - g(x)) = e^x + e^{-x} \] \[ 2f(x) = e^x + e^{-x} \] Recall that the sum of exponential terms is the definition of the hyperbolic cosine function: \[ e^x + e^{-x} = 2\cosh(x), \] so we have: \[ 2f(x) = 2\cosh(x) \quad \Rightarrow \quad f(x) = \cosh(x). \] Since \( \cosh(x) \) is an even function (i.e., \( \cosh(-x) = \cosh(x) \)), it follows that \( f(x) \) is an even function.
Step 2: Subtract the two equations.
Next, subtract the second equation from the first: \[ (f(x) + g(x)) - (f(x) - g(x)) = e^x - e^{-x} \] \[ 2g(x) = e^x - e^{-x} \] The difference of the exponential terms is the definition of the hyperbolic sine function: \[ e^x - e^{-x} = 2\sinh(x), \] so we have: \[ 2g(x) = 2\sinh(x) \quad \Rightarrow \quad g(x) = \sinh(x). \] Since \( \sinh(x) \) is an odd function (i.e., \( \sinh(-x) = -\sinh(x) \)), it follows that \( g(x) \) is an odd function.
Step 3: Conclusion
Thus, we have determined that \( f(x) \) is an even function and \( g(x) \) is an odd function.
The maximum value of the function \( f(x) = (x - 1)(x - 2)(x - 3) \) in the domain [0, 3] occurs at \( x = \) _________ (rounded off to two decimal places).
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.