The values of X, Y, and Z in the following chemical equation are respectively: \( S_8 + X HNO_3 ({conc.}) \rightarrow Y H_2SO_4 + X NO_2 + Z H_2O \)
Which of the following changes alone would cause increase in the value of the equilibrium constant of the reaction? \(PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g); \Delta H>0\)
For the reaction:
$3Fe_{(s)} + 2O_2{(g)} \rightarrow Fe_3O_4{(s)}$
$\Delta H = -1650\,\text{kJ mol}^{-1}$, $\Delta S = -600\,\text{J K}^{-1} \text{mol}^{-1}$ at $300\,\text{K}$. What is the value of free energy change for the reaction at $300\,\text{K}$?
In Young’s double slit experiment, to change the bandwidth from $\beta$ to $\frac{\beta}{4}$ without changing the experimental setup, the wavelength of light $\lambda$ used must be changed to
\[ 2X(g) \rightleftharpoons 2Y(g) + Z(g) \]
\[ R = 0.082 \, \text{L atm K}^{-1} \, \text{mol}^{-1} \]