The relation between two specific heats (in cal/mol) of a gas is:
1.
2.
3.
4.
The ratio of the specific heats in terms of degrees of freedom (\(n\)) is given by:
1. \(1+1/n\)
2. \(1+n/3\)
3. \(1+2/n\)
4. \(1+n/2\)
The figure shows a process for a gas in which pressure (P) and volume (V) of the gas change. If and are the molar heat capacities of the gas during the processes AB and BC respectively, then:
1.
2.
3.
4.
If \(C_p\) and \(C_v\) denote the specific heats (per unit mass) of an ideal gas of molecular weight \(M\) (where \(R\) is the molar gas constant), the correct relation is:
1. \(C_p-C_v=R\)
2. \(C_p-C_v=\frac{R}{M}\)
3. \(C_p-C_v=MR\)
4. \(C_p-C_v=\frac{R}{M^2}\)
The specific heat of an ideal gas is:
1. proportional to
2. proportional to T2.
3. proportional to T3.
4. independent of
For hydrogen gas \(C_P-C_V=a\) and for oxygen gas \(C_P-C_V=b\) where molar specific heats are given. So the relation between \(a\) and \(b\) is given by: (where \(C_p\) and \(C_V\) in J mol-1 K-1)
1. \(a=16b\)
2. \(b=16a\)
3. \(a=4b\)
4. \(a=b\)
The specific heat of a gas:
1. | has only two values \(Cp\) and \(Cv\). |
2. | has a unique value at a given temperature. |
3. | can have any value between 0 and ∞. |
4. | depends upon the mass of the gas. |
The value of for a gas in state A and in another state B. If denote the pressure and denote the temperatures in the two states, then:
1. | \(P_A=P_B ; T_A>T_B\) |
2. | \(P_A>P_B ; T_A=T_B\) |
3. | \(P_A<P_B ; T_A>T_B\) |
4. | \(P_A=P_B ; T_A<T_B\) |
The amount of heat energy required to raise the temperature of \(1\) g of Helium at NTP, from \({T_1}\) K to \({T_2}\) K is:
1. \(\frac{3}{2}N_ak_B(T_2-T_1)\)
2. \(\frac{3}{4}N_ak_B(T_2-T_1)\)
3. \(\frac{3}{4}N_ak_B\frac{T_2}{T_1}\)
4. \(\frac{3}{8}N_ak_B(T_2-T_1)\)
A cylinder of fixed capacity \(44.8\) litres contains helium gas at standard temperature and pressure. What is the amount of heat needed to raise the temperature of the gas in the cylinder by \(15.0^\circ~\mathrm{C}?\) (\(R=8.31\) J mol–1 K–1)
1. | \(379\) J | 2. | \(357\) J |
3. | \(457\) J | 4. | \(374\) J |