To solve this problem, we need to determine the temperature \(t\) at which the resistance of a wire is \(10.95 \, \Omega\). We are given the resistance at \(0^\circ C\) is \(10 \, \Omega\) and at \(100^\circ C\) is \(10.2 \, \Omega\). The resistance \(R(t)\) of a wire at temperature \(t\) is given by: \[ R(t)=R_0(1+\alpha t) \] where \( R_0 \) is the resistance at \(0^\circ C\), \(\alpha\) is the temperature coefficient of resistance. **Step 1: Calculate \(\alpha\)** At \(100^\circ C\), we have: \[ 10.2 = 10(1 + 100\alpha) \] \[ 10.2 = 10 + 1000\alpha \] \[ 0.2 = 1000\alpha \] \[ \alpha = 0.0002 \] **Step 2: Find temperature \(t\) for resistance \(10.95 \, \Omega\)** Using the equation: \[ 10.95 = 10(1 + 0.0002t) \] \[ 10.95 = 10 + 0.002t \] \[ 0.95 = 0.002t \] \[ t = \frac{0.95}{0.002} \] \[ t = 475 \] **Step 3: Convert temperature to Kelvin scale** \[ t = 475^\circ C \] \[ T(K) = 475 + 273.15 = 748.15 \] **Step 4: Verify within range** Given the range (748, 748), \(T\) calculated as 748.15 falls within this range when rounded appropriately. Thus, the temperature \(t\) in Kelvin scale is approximately 748 K.
The temperature dependence of resistance is given by:
\[R = R_0 (1 + \alpha \Delta T).\]
From $0^\circ \text{C}$ to $100^\circ \text{C}$:
\[\frac{\Delta R}{R_0} = \alpha \Delta T \implies \alpha = \frac{10.2 - 10}{10 \cdot 100} = 0.002.\]
From $0^\circ \text{C}$ to $t^\circ \text{C}$:
\[\frac{\Delta R}{R_0} = \alpha \Delta T \implies \Delta T = \frac{10.95 - 10}{10 \cdot 0.002}.\]
\[\Delta T = 475^\circ \text{C}.\]
Convert to Kelvin:
T = 475 + 273 = 748 K
Final Answer: $748 \, \text{K}$.
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 : \(A_2 \rightleftharpoons 2A\)