\( 4 \)
\( 5 \)
Let the first term of the A.P. be \( a \) and the common difference be \( d \). The A.P. has \( 2k \) terms. The last term of the A.P. can be expressed as \( a + (2k-1)d \). According to the problem, this last term exceeds the first term by 27, so we have:
\( a + (2k-1)d = a + 27 \)
This simplifies to:
\( (2k-1)d = 27 \)
The sum of the odd terms \( a, a+2d, a+4d, \ldots \) consists of \( k \) terms. Using the sum formula for an A.P., the sum \( S_{\text{odd}} \) of these terms is given as 40:
\( S_{\text{odd}} = \frac{k}{2} \times [2a + (k-1)2d] = 40 \)
This can be rewritten as:
\( k(a + (k-1)d) = 40 \)
Similarly, the sum of the even terms \( a+d, a+3d, a+5d, \ldots \) also consists of \( k \) terms, and the sum \( S_{\text{even}} \) is given as 55:
\( S_{\text{even}} = \frac{k}{2} \times [2(a+d) + (k-1)2d] = 55 \)
This simplifies to:
\( k(a + kd) = 55 \)
Now, we have the following system of equations:
Simplifying the first equation, we have:
\( d = \frac{27}{2k-1} \)
Substitute \( d \) in the second equation:
\( k(a + (k-1)\frac{27}{2k-1}) = 40 \)
From the third equation, substituting \( d \):
\( k(a + k\frac{27}{2k-1}) = 55 \)
Subtract the second equation from the third:
\( k(k\frac{27}{2k-1} - (k-1)\frac{27}{2k-1}) = 15 \)
This reduces to:
\( k(\frac{27}{2k-1}) = 15 \)
Solving for \( k \), we substitute:
\( k = \frac{15(2k-1)}{27} \)
Simplifying:
\( 15(2k-1) = 27k \)
This simplifies to:
\( 30k - 15 = 27k \)
Therefore:
\( 3k = 15 \)
Thus:
\( k = 5 \)
Thus, the correct value of \( k \) that satisfies all conditions is 5.
Let \( \alpha, \beta \) be the roots of the equation \( x^2 - ax - b = 0 \) with \( \text{Im}(\alpha) < \text{Im}(\beta) \). Let \( P_n = \alpha^n - \beta^n \). If \[ P_3 = -5\sqrt{7}, \quad P_4 = -3\sqrt{7}, \quad P_5 = 11\sqrt{7}, \quad P_6 = 45\sqrt{7}, \] then \( |\alpha^4 + \beta^4| \) is equal to:
For the thermal decomposition of \( N_2O_5(g) \) at constant volume, the following table can be formed, for the reaction mentioned below: \[ 2 N_2O_5(g) \rightarrow 2 N_2O_4(g) + O_2(g) \] Given: Rate constant for the reaction is \( 4.606 \times 10^{-2} \text{ s}^{-1} \).
O\(_2\) gas will be evolved as a product of electrolysis of:
(A) an aqueous solution of AgNO3 using silver electrodes.
(B) an aqueous solution of AgNO3 using platinum electrodes.
(C) a dilute solution of H2SO4 using platinum electrodes.
(D) a high concentration solution of H2SO4 using platinum electrodes.
Choose the correct answer from the options given below :