If the system of equations: $$ \begin{aligned} 3x + y + \beta z &= 3 \\2x + \alpha y + z &= 2 \\x + 2y + z &= 4 \end{aligned} $$ has infinitely many solutions, then the value of \( 22\beta - 9\alpha \) is:
For infinitely many solutions, the rank of the coefficient matrix and the augmented matrix must be equal and less than the number of variables. Using determinant conditions:
\[ \Delta = \begin{vmatrix} 3 & 1 & \beta 2 & \alpha & 1 \\ 1 & 2 & 1 \end{vmatrix} = 0 \quad \text{and} \quad \Delta_3 = \begin{vmatrix} 3 & 1 & 3\\ 2 & \alpha & 2 \\1 & 2 & 4 \end{vmatrix} = 0 \] Solving gives \( \alpha = \frac{19}{9}, \beta = \frac{6}{11} \), so: \[ 22\beta - 9\alpha = 31 \]
Consider the matrix:
\[ A = \begin{bmatrix} 2 & 3 \\ 1 & 2 \end{bmatrix} \]
The eigenvalues of the matrix are 0.27 and ____ (rounded off to 2 decimal places).
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.