\( \frac{12}{35} \)
We are given two bags: - Bag \( P \) contains:
- 3 white balls
- 2 red balls
- 5 blue balls
- Bag \( Q \) contains:
- 2 white balls
- 3 red balls
- 5 blue balls
A ball is first chosen randomly from Bag \( P \) and placed into Bag \( Q \). Then, a ball is randomly selected from Bag \( Q \). We need to determine the probability that the selected ball from Bag \( Q \) is red.
Step 1: Define Probabilities for Transfer from \( P \) Since a ball is chosen at random from Bag \( P \): \[ P(\text{white}) = \frac{3}{10}, \quad P(\text{red}) = \frac{2}{10}, \quad P(\text{blue}) = \frac{5}{10} \]
Step 2: Update Bag \( Q \) Based on Transfer 1. If a white ball is transferred: - Bag \( Q \) now has 3 white, 3 red, 5 blue. - Probability of selecting a red ball from \( Q \): \[ P(R | W) = \frac{3}{(2+1+3+5)} = \frac{3}{11} \] 2. If a red ball is transferred:
- Bag \( Q \) now has 2 white, 4 red, 5 blue.
- Probability of selecting a red ball from \( Q \): \[ P(R | R) = \frac{4}{(2+3+1+5)} = \frac{4}{11} \] 3. If a blue ball is transferred: - Bag \( Q \) now has 2 white, 3 red, 6 blue. - Probability of selecting a red ball from \( Q \): \[ P(R | B) = \frac{3}{(2+3+5+1)} = \frac{3}{11} \]
Step 3: Compute Total Probability Using Law of Total Probability \[ P(R) = P(W) P(R | W) + P(R) P(R | R) + P(B) P(R | B) \] \[ = \left(\frac{3}{10} \times \frac{3}{11} \right) + \left(\frac{2}{10} \times \frac{4}{11} \right) + \left(\frac{5}{10} \times \frac{3}{11} \right) \] \[ = \frac{9}{110} + \frac{8}{110} + \frac{15}{110} \] \[ = \frac{32}{110} = \frac{16}{55} \]
Final Answer: \(\boxed{\frac{16}{55}}\)
Observe the following data given in the table. (\(K_H\) = Henry's law constant)
Gas | CO₂ | Ar | HCHO | CH₄ |
---|---|---|---|---|
\(K_H\) (k bar at 298 K) | 1.67 | 40.3 | \(1.83 \times 10^{-5}\) | 0.413 |
The correct order of their solubility in water is
For a first order decomposition of a certain reaction, rate constant is given by the equation
\(\log k(s⁻¹) = 7.14 - \frac{1 \times 10^4 K}{T}\). The activation energy of the reaction (in kJ mol⁻¹) is (\(R = 8.3 J K⁻¹ mol⁻¹\))
Note: The provided value for R is 8.3. We will use the more precise value R=8.314 J K⁻¹ mol⁻¹ for accuracy, as is standard.