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Q. No.An ideal gas has molecules with \(5\) degrees of freedom. The ratio of specific heats at constant pressure \(C_{P}\) and at constant volume \(C_V\) is:
1. \(\frac{7}{2}\)
2. \(\frac{7}{5}\)
3. \(6\)
4. \(\frac{5}{2}\)
1. \(\frac{7}{2}\)
2. \(\frac{7}{5}\)
3. \(6\)
4. \(\frac{5}{2}\)
Subtopic: Specific Heat |
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The total internal energy of two moles of a monoatomic ideal gas at temperature \(T = 300~\text{K}\) will be:
(Given: \(R = 8.31\) J/mol.K)
1. \(4789~\text{J}\)
2. \(7479~\text{J}\)
3. \(5896~\text{J}\)
4. \(8346~\text{J}\)
(Given: \(R = 8.31\) J/mol.K)
1. \(4789~\text{J}\)
2. \(7479~\text{J}\)
3. \(5896~\text{J}\)
4. \(8346~\text{J}\)
Subtopic: Specific Heat |
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A gas has \(n\) degrees of freedom. The ratio of the specific heat of the gas at constant volume to the specific heat of the gas at constant pressure will be:
| 1. | \({\dfrac{n} {n+2}}\) | 2. | \({\dfrac{n+2} {n}}\) |
| 3. | \({\dfrac{n} {2n+2}}\) | 4. | \({\dfrac{n} {n-2}}\) |
Subtopic: Specific Heat |
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One mole of a monoatomic gas is mixed with three moles of a diatomic gas. If the molecular specific heat of the mixture at constant volume is \(\dfrac{\alpha^2}{4} {R}~ \text{J} / \text{mol-K},\) then the value of \(\alpha\) will be:
(assume that the given diatomic gas has no vibrational mode)
(assume that the given diatomic gas has no vibrational mode)
| 1. | \(5\) | 2. | \(4\) |
| 3. | \(3\) | 4. | \(2\) |
Subtopic: Specific Heat |
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\(N\) moles of non-linear polyatomic gas (degree of freedom \(6\)) is mixed with \(2\) moles of monoatomic gas. The resultant mixture has molar-specific heat equal to that of a diatomic gas, then the number of moles \((N)\) is:
1. \(4\)
2. \(5\)
3. \(6\)
4. \(3\)
1. \(4\)
2. \(5\)
3. \(6\)
4. \(3\)
Subtopic: Specific Heat |
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A mixture contains one mole of a monoatomic gas and one mole of a rigid diatomic gas at room temperature \(\left(27^{\circ} \mathrm{C}\right). \) What is the ratio of their specific heats at constant volume?
| 1. | \(\dfrac{3}{2}\) | 2. | \(\dfrac{7}{5}\) |
| 3. | \(\dfrac{3}{5}\) | 4. | \(\dfrac{5}{2}\) |
Subtopic: Specific Heat |
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Two moles of an ideal gas with \(\frac{C_P}{C_V}=\frac{5}{3}\) are mixed with \(3\) moles of another ideal gas with \(\frac{{C}_{{P}}}{{C}_{{V}}}=\frac{4}{3}.\) The value of \(\frac{{C}_{P}}{{C}_{V}}\) for the mixture is:
1. \(1.42\)
2. \(1.47\)
3. \(1.45\)
4. \(1.50\)
1. \(1.42\)
2. \(1.47\)
3. \(1.45\)
4. \(1.50\)
Subtopic: Specific Heat |
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Consider a mixture of \(n\) moles of helium gas and \(2n\) moles of oxygen gas (molecules taken to be rigid) as an ideal gas. Its \(\dfrac{C_p}{C_v}\) value is:
| 1. | \(\dfrac{19}{13}\) | 2. | \(\dfrac{40}{27}\) |
| 3. | \(\dfrac{67}{45}\) | 4. | \(\dfrac{23}{15}\) |
Subtopic: Specific Heat |
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Consider two ideal diatomic gases \(A\) and \(B\) at same temperature \(T.\) The molecules of gas \(A\) are rigid, and have a mass of \(m.\) The molecules of gas \(B\) have an additional vibrational mode and have a mass of \(\dfrac{m}{4}.\) The ratio of their specific heats \(\left(C_vA\right) \) and \(\left(C_vB\right)\) of gas \(A\) and \(B,\) is:
1. \(3: 5\)
2. \(5: 7\)
3. \(7: 9\)
4. \(5: 9\)
1. \(3: 5\)
2. \(5: 7\)
3. \(7: 9\)
4. \(5: 9\)
Subtopic: Specific Heat |
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