We are given the integral \[ I = \int_0^{\pi} \frac{x \sin x}{4 \cos^2 x + 3 \sin^2 x} dx. \]
Step 1: Simplify the denominator using a standard trigonometric identity: \[ 4 \cos^2 x + 3 \sin^2 x = 4 - \sin^2 x. \]
Step 2: The integral can be simplified further, but we can use known results for trigonometric integrals to directly obtain: \[ I = \frac{\pi^2}{6\sqrt{3}}. \] Thus, the correct answer is \( \frac{\pi^2}{6\sqrt{3}} \).
Let \[ f(t)=\int \left(\frac{1-\sin(\log_e t)}{1-\cos(\log_e t)}\right)dt,\; t>1. \] If $f(e^{\pi/2})=-e^{\pi/2}$ and $f(e^{\pi/4})=\alpha e^{\pi/4}$, then $\alpha$ equals
Let $(2\alpha,\alpha)$ be the largest interval in which the function \[ f(t)=\frac{|t+1|}{t^2},\; t<0 \] is strictly decreasing. Then the local maximum value of the function \[ g(x)=2\log_e(x-2)+\alpha x^2+4x-\alpha,\; x>2 \] is
Which of the following are ambident nucleophiles?
[A.] CN$^{\,-}$
[B.] CH$_{3}$COO$^{\,-}$
[C.] NO$_{2}^{\,-}$
[D.] CH$_{3}$O$^{\,-}$
[E.] NH$_{3}$
Identify the anomers from the following.

The standard Gibbs free energy change \( \Delta G^\circ \) of a cell reaction is \(-301 { kJ/mol}\). What is \( E^\circ \) in volts?
(Given: \( F = 96500 { C/mol}\), \( n = 2 \))