We are given the series: \[ S_n = \frac{1}{1.5} + \frac{1}{5.9} + \frac{1}{9.13} + \cdots \quad \text{up to \( n \) terms}. \] First, observe the pattern in the denominators. The terms in the denominators follow a sequence of the form: \[ 1.5, 5.9, 9.13, \cdots \] This suggests that the general form of the denominator for the \( k \)-th term is: \[ (4k - 2) + 0.5 \] Thus, the \( k \)-th term of the series can be written as: \[ T_k = \frac{1}{(4k - 2) + 0.5} = \frac{1}{4k + 1}. \] Step 1: The sum of the series up to \( n \) terms is: \[ S_n = \sum_{k=1}^{n} \frac{1}{4k + 1}. \] This simplifies to: \[ S_n = \frac{1}{4(1) + 1} + \frac{1}{4(2) + 1} + \frac{1}{4(3) + 1} + \cdots + \frac{1}{4n + 1}. \]
Step 2: The general formula for the sum of this series up to \( n \) terms is: \[ S_n = \frac{n}{4n + 1}. \] Thus, the sum of the series is \( \frac{n}{4n + 1} \).
The value of $\lim_{n \to \infty} \sum_{k=1}^{n} \frac{k^3 + 6k^2 + 11k + 5}{(k+3)!}$ 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: \( F = 96500 { C/mol}\), \( n = 2 \))