Step 1: Form the augmented matrix of the system
The given system of equations can be written as the augmented matrix: \[ \Delta = \begin{vmatrix} 6\lambda & -3 & 3 2 & 6\lambda & 4 3 & 2 & 3\lambda \end{vmatrix} \] For the system to have no solution, the determinant of the coefficient matrix must be zero.
Step 2: Calculate the determinant We calculate the determinant \( \Delta \): \[ \Delta = 6\lambda \begin{vmatrix} 6\lambda & 4 2 & 3\lambda \end{vmatrix} - (-3) \begin{vmatrix} 2 & 4 3 & 3\lambda \end{vmatrix} + 3 \begin{vmatrix} 2 & 6\lambda 3 & 2 \end{vmatrix} \] Simplifying the 2x2 determinants: \[ \Delta = 6\lambda \left( (6\lambda)(3\lambda) - (4)(2) \right) + 3 \left( (2)(3\lambda) - (4)(3) \right) + 3 \left( (2)(2) - (6\lambda)(3) \right) \] \[ \Delta = 6\lambda \left( 18\lambda^2 - 8 \right) + 3 \left( 6\lambda - 12 \right) + 3 \left( 4 - 18\lambda \right) \] Expanding the terms: \[ \Delta = 6\lambda (18\lambda^2 - 8) + 3(6\lambda - 12) + 3(4 - 18\lambda) \] \[ \Delta = 108\lambda^3 - 48\lambda + 18\lambda - 36 + 12 - 54\lambda \] \[ \Delta = 108\lambda^3 - 84\lambda - 24 \]
Step 3: Solve for \( \lambda \)
For the system to have no solution, the determinant must be zero: \[ 108\lambda^3 - 84\lambda - 24 = 0 \] Divide the entire equation by 12: \[ 9\lambda^3 - 7\lambda - 2 = 0 \]
Step 4: Find the roots of the cubic equation Solving the cubic equation \( 9\lambda^3 - 7\lambda - 2 = 0 \) by using trial and error or factoring, we find the roots: \[ \lambda = 1, -\frac{1}{3}, \frac{2}{3} \]
Step 5: Calculate \( 12 \sum_{\lambda \in S} |\lambda| \)
Now, the values of \( \lambda \) are \( 1, -\frac{1}{3}, \frac{2}{3} \). The sum of their absolute values is: \[ |1| + \left| -\frac{1}{3} \right| + \left| \frac{2}{3} \right| = 1 + \frac{1}{3} + \frac{2}{3} = 2 \] Thus, \[ 12 \sum_{\lambda \in S} |\lambda| = 12 \times 2 = 24 \] Thus, the required value is \( \boxed{24} \).
What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)
A black body is at a temperature of 2880 K. The energy of radiation emitted by this body with wavelength between 499 nm and 500 nm is U1, between 999 nm and 1000 nm is U2 and between 1499 nm and 1500 nm is U3. The Wien's constant, b = 2.88×106 nm-K. Then,