Given Function:
\(f(x) = \lfloor a + 13 \sin x \rfloor\) for \(x \in (0, \pi)\), where \(a\) is an integer and \(\lfloor t \rfloor\) is the greatest integer less than or equal to \(t\).
Since \(0 < x < \pi\), we have \(0 < \sin x \leq 1\), and thus \(0 < 13 \sin x \leq 13\).
The greatest integer function is discontinuous at integer values of \(x\). So, \(\lfloor 13 \sin x \rfloor\) will be discontinuous when \(13 \sin x\) takes integer values from 1 to 13.
For each integer \(k\) from 1 to 12, the equation \(13 \sin x = k\) has two solutions in the interval \((0, \pi)\).
The equation \(13 \sin x = 13\) has only one solution in the interval \((0, \pi)\), which is \(x = \frac{\pi}{2}\).
Therefore, the number of points of discontinuity is:
\[ 2 \times 12 + 1 = 25 \]
The function \(f(x)\) is not differentiable at 25 points in \((0, \pi)\).
For \( n \in \mathbb{N} \), the largest positive integer that divides \( 81^n + 20n - 1 \) is \( k \). If \( S \) is the sum of all positive divisors of \( k \), then find \( S - k \).
Consider the following reaction occurring in the blast furnace. \[ {Fe}_3{O}_4(s) + 4{CO}(g) \rightarrow 3{Fe}(l) + 4{CO}_2(g) \] ‘x’ kg of iron is produced when \(2.32 \times 10^3\) kg \(Fe_3O_4\) and \(2.8 \times 10^2 \) kg CO are brought together in the furnace.
The value of ‘x’ is __________ (nearest integer).
Among the following cations, the number of cations which will give characteristic precipitate in their identification tests with
\(K_4\)[Fe(CN)\(_6\)] is : \[ {Cu}^{2+}, \, {Fe}^{3+}, \, {Ba}^{2+}, \, {Ca}^{2+}, \, {NH}_4^+, \, {Mg}^{2+}, \, {Zn}^{2+} \]
X g of benzoic acid on reaction with aqueous \(NaHCO_3\) release \(CO_2\) that occupied 11.2 L volume at STP. X is ________ g.
Standard entropies of \(X_2\), \(Y_2\) and \(XY_5\) are 70, 50, and 110 J \(K^{-1}\) mol\(^{-1}\) respectively. The temperature in Kelvin at which the reaction \[ \frac{1}{2} X_2 + \frac{5}{2} Y_2 \rightarrow XY_5 \quad \Delta H = -35 \, {kJ mol}^{-1} \] will be at equilibrium is (nearest integer):
37.8 g \( N_2O_5 \) was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K: \[ 2N_2O_5(g) \rightarrow 2N_2O_4(g) + O_2(g) \]
The total pressure at equilibrium was found to be 18.65 bar. Then, \( K_p \) is: Given: \[ R = 0.082 \, \text{bar L mol}^{-1} \, \text{K}^{-1} \]