If the system of equation $$ 2x + \lambda y + 3z = 5 \\3x + 2y - z = 7 \\4x + 5y + \mu z = 9 $$ has infinitely many solutions, then $ \lambda^2 + \mu^2 $ is equal to:
The given system of equations is: \[ 2x + \lambda y + 3z = 5 3x + 2y - z = 7 \\4x + 5y + \mu z = 9 \] To check for infinitely many solutions, we use the determinant of the coefficient matrix. The coefficient matrix is: \[ \Delta = \begin{vmatrix} 2 & \lambda & 3 3 & 2 & -1 \\ 4 & 5 & \mu \end{vmatrix} \] \[ \Delta = 0 \quad \text{(for infinitely many solutions)} \] Expanding the determinant: \[ \Delta = 2 \begin{vmatrix} 2 & -1 5 & \mu \end{vmatrix} - \lambda \begin{vmatrix} 3 & -1 \\ 4 & \mu \end{vmatrix} + 3 \begin{vmatrix} 3 & 2 \\ 4 & 5 \end{vmatrix} \] \[ = 2(\lambda \mu - (-5)) - \lambda (3 \mu - (-4)) + 3(15 - 8) \] \[ = 2(\lambda \mu + 5) - \lambda (3 \mu + 4) + 3(7) \] \[ = 2\lambda \mu + 10 - \lambda (3 \mu + 4) + 21 \] \[ = 2\lambda \mu + 10 - \lambda 3 \mu - 4 \lambda + 21 \] After solving the system, we find: \[ \Delta_3 = 0 \quad \text{and} \quad 2(7) + \lambda(1) + 5(7) = 0 \] Solving for \( \lambda \) and \( \mu \), we find \( \lambda = -1 \) and \( \mu = -5 \). Hence, \[ \lambda^2 + \mu^2 = (-1)^2 + (-5)^2 = 1 + 25 = 26 \]
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.