Let $ A = \begin{bmatrix} \alpha & -1 \\6 & \beta \end{bmatrix},\ \alpha > 0 $, such that $ \det(A) = 0 $ and $ \alpha + \beta = 1 $. If $ I $ denotes the $ 2 \times 2 $ identity matrix, then the matrix $ (1 + A)^5 $ is:
\( \begin{bmatrix} 4 & -1 \\6 & -1 \end{bmatrix} \)
\( \begin{bmatrix} 257 & -64 \\514 & -127 \end{bmatrix} \)
\( \begin{bmatrix} 1025 & -511 \\2024 & -1024 \end{bmatrix} \)
\( \begin{bmatrix} 766 & -255 \\1530 & -509 \end{bmatrix} \)
From \( \det(A) = \alpha \beta + 6 = 0 \), we get \( \alpha \beta = -6 \), and \( \alpha + \beta = 1 \). Solving: \[ \alpha = 3,\quad \beta = -2 \Rightarrow A = \begin{bmatrix} 3 & -1 6 & -2 \end{bmatrix} \] Check powers: \[ A^2 = A \Rightarrow A^n = A,\ \forall n \geq 1 \] Use binomial expansion: \[ (1 + A)^5 = I + 5A + 10A^2 + 10A^3 + 5A^4 + A^5 = I + 31A \] \[ (1 + A)^5 = \begin{bmatrix} 1 & 0 0 & 1 \end{bmatrix} + 31 \cdot \begin{bmatrix} 3 & -1 \\6 & -2 \end{bmatrix} = \begin{bmatrix} 766 & -255 \\1530 & -509 \end{bmatrix} \]
Let $A = \begin{bmatrix} \cos \theta & 0 & -\sin \theta \\ 0 & 1 & 0 \\ \sin \theta & 0 & \cos \theta \end{bmatrix}$. If for some $\theta \in (0, \pi)$, $A^2 = A^T$, then the sum of the diagonal elements of the matrix $(A + I)^3 + (A - I)^3 - 6A$ is equal to
Let $ A $ be a $ 3 \times 3 $ matrix such that $ | \text{adj} (\text{adj} A) | = 81.
$ If $ S = \left\{ n \in \mathbb{Z}: \left| \text{adj} (\text{adj} A) \right|^{\frac{(n - 1)^2}{2}} = |A|^{(3n^2 - 5n - 4)} \right\}, $ then the value of $ \sum_{n \in S} |A| (n^2 + n) $ is:
A molecule with the formula $ \text{A} \text{X}_2 \text{Y}_2 $ has all it's elements from p-block. Element A is rarest, monotomic, non-radioactive from its group and has the lowest ionization energy value among X and Y. Elements X and Y have first and second highest electronegativity values respectively among all the known elements. The shape of the molecule is:
A transition metal (M) among Mn, Cr, Co, and Fe has the highest standard electrode potential $ M^{n}/M^{n+1} $. It forms a metal complex of the type $[M \text{CN}]^{n+}$. The number of electrons present in the $ e $-orbital of the complex is ... ...
Consider the following electrochemical cell at standard condition. $$ \text{Au(s) | QH}_2\text{ | QH}_X(0.01 M) \, \text{| Ag(1M) | Ag(s) } \, E_{\text{cell}} = +0.4V $$ The couple QH/Q represents quinhydrone electrode, the half cell reaction is given below: $$ \text{QH}_2 \rightarrow \text{Q} + 2e^- + 2H^+ \, E^\circ_{\text{QH}/\text{Q}} = +0.7V $$
0.1 mol of the following given antiviral compound (P) will weigh .........x $ 10^{-1} $ g.
Consider the following equilibrium, $$ \text{CO(g)} + \text{H}_2\text{(g)} \rightleftharpoons \text{CH}_3\text{OH(g)} $$ 0.1 mol of CO along with a catalyst is present in a 2 dm$^3$ flask maintained at 500 K. Hydrogen is introduced into the flask until the pressure is 5 bar and 0.04 mol of CH$_3$OH is formed. The $ K_p $ is ...... x $ 10^7 $ (nearest integer).
Given: $ R = 0.08 \, \text{dm}^3 \, \text{bar} \, \text{K}^{-1} \, \text{mol}^{-1} $
Assume only methanol is formed as the product and the system follows ideal gas behavior.