The condition for two lines to be coplanar is that the scalar triple product of the direction ratios of the two lines, along with the vector joining any two points on the lines, must be zero.
We are given the first line in symmetric form: \[ \frac{x+3}{-3} = \frac{y-1}{1} = \frac{z-5}{5} \] The direction ratios of this line are \( \mathbf{a_1} = (-3, 1, 5) \). Let’s calculate the condition for coplanarity.
The second line is of the form: \[ \frac{x+1}{-1} = \frac{y-2}{2} = \frac{z-5}{5} \] The direction ratios of the second line are \( \mathbf{a_2} = (-1, 2, 5) \). Now, to check for coplanarity, we apply the condition of coplanarity for two lines.
The condition involves the scalar triple product of the direction ratios of the two lines and the vector joining any point on the first line to a point on the second line.
Let’s take points on the lines: - For the first line, take \( P_1(-3, 1, 5) \).
- For the second line, take \( P_2(-1, 2, 5) \). The vector joining these points is \( \overrightarrow{P_1P_2} = (-1 - (-3), 2 - 1, 5 - 5) = (2, 1, 0) \).
The scalar triple product condition for coplanarity is: \[ \left| \begin{matrix} x_2 - x_1 & a_1 & a_2 y_2 - y_1 & b_1 & b_2 z_2 - z_1 & c_1 & c_2 \end{matrix} \right| = 0 \]
Substitute the values into the determinant: \[ \begin{vmatrix} 2 & -3 & -1 1 & 1 & 2 0 & 5 & 5 \end{vmatrix} \]
Now, calculate the determinant: \[ = 2 \begin{vmatrix} 1 & 2 5 & 5 \end{vmatrix} - (-3) \begin{vmatrix} 1 & 2 0 & 5 \end{vmatrix} + (-1) \begin{vmatrix} 1 & 1 0 & 5 \end{vmatrix} \] \[ = 2 \left( (1 \times 5) - (2 \times 5) \right) + 3 \left( (1 \times 5) - (2 \times 0) \right) + (-1) \left( (1 \times 5) - (1 \times 0) \right) \] \[ = 2 \left( 5 - 10 \right) + 3 \left( 5 - 0 \right) + (-1) \left( 5 - 0 \right) \] \[ = 2(-5) + 3(5) - 1(5) \] \[ = -10 + 15 - 5 = 0 \] Since the determinant is zero, the two lines are coplanar.
Thus, the correct option is (2).
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,