Mass of nitrogen, m = 2.0 × 10-2 kg=20 g
in temperature, ΔT = 45°C
Molecular mass of N2, M = 28
Universal gas constant, R = 8.3 J mol-1 k-1
Number of moles, \(n=\frac{m}{M}\)
\(=\frac{2.0×10^{-2}×10^3}{28}=0.714\)
Molar specific heat at constant pressure for nitrogen, \(c_p=\frac{7}{2}\,R\)
\(=\frac{7}{2}×8.3\)
=29.05 J mol-1 K-1
The total amount of heat to be supplied is given by the relation:
\(ΔQ = C_p^n ΔT\)
\(= 0.714 × 29.05 × 45\)
\( = 933.38 \,J\)
Therefore, the amount of heat to be supplied is 933.38 J.
In the given cycle ABCDA, the heat required for an ideal monoatomic gas will be:
Three identical rods are joined as shown in the figure. The left and right ends are kept at \( 0^\circ C \) and \( 90^\circ C \) as shown in the figure. The temperature \( \theta \) at the junction of the rods is:
List-I | List-II | ||
P | The value of \(I1\) in Ampere is | I | \(0\) |
Q | The value of I2 in Ampere is | II | \(2\) |
R | The value of \(\omega_0\) in kilo-radians/s is | III | \(4\) |
S | The value of \(V_0\) in Volt is | IV | \(20\) |
200 |
What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions?