To solve this problem, we need to determine the number of moles \(N\) of a polyatomic gas with degrees of freedom \(f = 6\) that must be mixed with two moles of a monoatomic gas (which has degrees of freedom \(f = 3\)) so that the mixture behaves like a diatomic gas (which has degrees of freedom \(f = 5\)).
The degrees of freedom \(f\) for a mixture of gases can be determined using the formula:
\(f_{\text{mix}} = \frac{N_1 \cdot f_1 + N_2 \cdot f_2}{N_1 + N_2}\)
where:
We are given:
Substituting these values into the formula:
\(5 = \frac{N \cdot 6 + 2 \cdot 3}{N + 2}\)
We solve for \(N\):
\(5(N + 2) = 6N + 6\)
Expanding both sides:
\(5N + 10 = 6N + 6\)
Rearranging the equation:
\(5N + 10 - 6 = 6N\)
\(5N + 4 = 6N\)
Simplify to solve for \(N\):
\(4 = 6N - 5N\)
\(N = 4\)
Thus, the value of \(N\) that satisfies this condition is 4. Therefore, the correct answer is 4.
The average degrees of freedom for the mixture, \( f_{\text{eq}} \), can be expressed as:
\(f_{\text{eq}} = \frac{n_1 f_1 + n_2 f_2}{n_1 + n_2}\)
where:
- \( n_1 = N \) (number of moles of polyatomic gas),
- \( n_2 = 2 \) (number of moles of monoatomic gas),
- \( f_1 = 6 \) (degrees of freedom for polyatomic gas),
- \( f_2 = 3 \) (degrees of freedom for monoatomic gas),
- \( f_{\text{eq}} = 5 \) (degrees of freedom for diatomic gas).
Now, we substitute these values into the equation:
\(5 = \frac{N \times 6 + 2 \times 3}{N + 2}\)
Simplify the equation:
\(5 = \frac{6N + 6}{N + 2}\)
Multiply both sides by \( (N + 2) \):
\(5(N + 2) = 6N + 6\)
\(5N + 10 = 6N + 6\)
\(10 - 6 = 6N - 5N\)
\(N = 4\)
Thus, the value of \( N \) is 4.
The Correct Answer is: 4
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,




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 : \(A_2 \rightleftharpoons 2A\)