If the probability density function of a random variable is given by $$ f(x) = \begin{cases} 12x^2(1 - x), & 0 \leq x \leq 1 \\ 0, & \text{elsewhere} \end{cases} $$ then the mean and variance are respectively:
The mean \( \mu \) of a random variable is given by:
\[ \mu = \int_0^1 x f(x) \, dx = \int_0^1 x \cdot 12x^2(1 - x) \, dx = \int_0^1 12x^3(1 - x) \, dx. \] Expanding the integrand: \[ \mu = 12 \int_0^1 (x^3 - x^4) \, dx = 12 \left[ \frac{x^4}{4} - \frac{x^5}{5} \right]_0^1 = 12 \left( \frac{1}{4} - \frac{1}{5} \right) = 12 \times \frac{1}{20} = 0.6. \] Now, the variance \( \sigma^2 \) is given by:
\[ \sigma^2 = \int_0^1 x^2 f(x) \, dx - \mu^2. \] First, compute the second moment: \[ \int_0^1 x^2 f(x) \, dx = \int_0^1 x^2 \cdot 12x^2(1 - x) \, dx = \int_0^1 12x^4(1 - x) \, dx. \] Expanding the integrand: \[ \int_0^1 12x^4(1 - x) \, dx = 12 \int_0^1 (x^4 - x^5) \, dx = 12 \left[ \frac{x^5}{5} - \frac{x^6}{6} \right]_0^1 = 12 \left( \frac{1}{5} - \frac{1}{6} \right) = 12 \times \frac{1}{30} = 0.4. \] Thus, the variance is: \[ \sigma^2 = 0.4 - (0.6)^2 = 0.4 - 0.36 = 0.04. \] Thus, the mean is \( 0.4 \) and the variance is \( 0.6 \).
A shop selling electronic items sells smartphones of only three reputed companies A, B, and C because chances of their manufacturing a defective smartphone are only 5%, 4%, and 2% respectively. In his inventory, he has 25% smartphones from company A, 35% smartphones from company B, and 40% smartphones from company C.
A person buys a smartphone from this shop
At 15 atm pressure, $ \text{NH}_3(g) $ is being heated in a closed container from 27°C to 347°C and as a result, it partially dissociates following the equation: $ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) $ If the volume of the container remains constant and pressure increases to 50 atm, then calculate the percentage dissociation of $ \text{NH}_3(g) $
If equilibrium constant for the equation $ A_2 + B_2 \rightleftharpoons 2AB \quad \text{is} \, K_p, $ then find the equilibrium constant for the equation $ AB \rightleftharpoons \frac{1}{2} A_2 + \frac{1}{2} B_2. $
Consider the following reaction: $ \text{CO}(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) $ At 27°C, the standard entropy change of the process becomes -0.094 kJ/mol·K. Moreover, standard free energies for the formation of $ \text{CO}_2(g) $ and $ \text{CO}(g) $ are -394.4 and -137.2 kJ/mol, respectively. Predict the nature of the above chemical reaction.