\(t_{\frac{1}{2}}∝\frac{1}{|P_o|^{n-1}}\)
\(\frac{(t_{1/2})_1}{(t_{1/2})}=\frac{|P_0|_2^{n-1}}{|P_0|_1^{n-1}}\)
\(\frac{340}{170}=(\frac{27.8}{55.5})^{n-1}\)
\(2=(\frac{1}{2})^{n-1}\)
2 = (2)1 – n
1 – n = 1
n = 0
At T(K), 0.1 moles of a non-volatile solute was dissolved in 0.9 moles of a volatile solvent. The vapour pressure of pure solvent is 0.9 . What is the vapour pressure (in ) of the solution?
The correct order of boiling points of hydrogen halides is:
The reaction:
\[ \text{H}_2\text{O}(g) + \text{Cl}_2\text{O}(g) \rightleftharpoons 2 \text{HOCl}(g) \]
is allowed to attain equilibrium at 400K. At equilibrium, the partial pressures are given as:
The value of \( K_p \) for the reaction at 400K is:
\[ K_p = \frac{P_{\text{HOCl}}^2}{P_{\text{H}_2\text{O}} \cdot P_{\text{Cl}_2\text{O}}} \]
The amount of time taken for half of a particular sample to react is known as Half-life.
We can describe exponential decay by any of the three formulas