Step 1: Rewrite the given differential equation:2(y+2)loge(y+2)dx+(x+4−2loge(y+2))dy=0
Step 2: Separate the variables:x+4−2loge(y+2)2(y+2)loge(y+2)dx=−dy
Step 3: Integrate both sides:∫x+4−2loge(y+2)2(y+2)loge(y+2)dx=−∫dy
Step 4: Use the initial condition x(e4−2)=1 to find the constant of integration.
Step 5: Solve for the particular solution using the initial condition.
Step 6: Evaluate the particular solution at y=e9−2 to find x(e9−2).
Final Answer: C. $\frac{32}{9}$
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 : \(A_2 \rightleftharpoons 2A\)
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,