Chromium metal can be plated out from an acidic solution containing ${\mathrm{CrO}}_3$ according to the following equation:${\mathrm{CrO}}_3 \left(\mathrm{aq}\right)+6{\mathrm{H}}^{+} \left(\mathrm{aq}\right)+6{\mathrm{e}}^{-}\to \mathrm{Cr} \left(\mathrm{s}\right)+3{\mathrm{H}}_2\mathrm{O}$

Calculate how long in (sec.) will it take to plate out $1.5 \mathrm{g}$ of chromium by using $12.5 \mathrm{amp.}$ current?

In starting a car, the battery delivers roughly $50$ amperes.

(i) During the $5$ seconds that it might take to start a car, totally how many grams of $\mathrm{Pb}$ and ${\mathrm{PbO}}_2$ are consumed in the battery?

(ii) If the car were run strictly from batteries, totally how many grams of $\mathrm{Pb}$ and ${\mathrm{PbO}}_2$ would be consumed per mile if $50$amperes made it go at $5 \mathrm{mph}$? The cell reaction is $\mathrm{Pb}+{\mathrm{PbO}}_2+2{\mathrm{H}}_2{\mathrm{SO}}_4\to 2{\mathrm{PbSO}}_4+2{\mathrm{H}}_2\mathrm{O}$.

The total pressure at equilibrium of a mixture of ${\mathrm{SO}}_2$ and ${\mathrm{O}}_2$ in the molar ratio $2:1$ when kept over a platinum catalyst at $723 \mathrm{K}$ is $10 \mathrm{atm}$. If $60\%$ of ${\mathrm{SO}}_2$ is converted into ${\mathrm{SO}}_3$, calculate ${\mathrm{K}}_{\mathrm{p}}$ for the reaction $\left(\mathrm{in} {\mathrm{atm}}^{-1}\right)$

$2{\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$

What would be the partial pressure of oxygen gas to get the equal partial pressure of ${\mathrm{SO}}_2$ and ${\mathrm{SO}}_3$?

$2{\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$

Given that the equilibrium partial pressures of ${\mathrm{SO}}_2, {\mathrm{O}}_2$ and ${\mathrm{SO}}_3$ are $0.662 \mathrm{atm}$, $0.101 \mathrm{atm}$ and $0.331 \mathrm{atm}$, respectively.

The value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction ${\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3+{\mathrm{Cl}}_2$ is $1.78$ at $250°\mathrm{C}$. Calculate the moles of ${\mathrm{PCl}}_5$ vapor dissociated at equilibrium when $0.40$ mole of ${\mathrm{PCl}}_5$ is vaporized in a vessel containing $0.20$ mole of ${\mathrm{Cl}}_2$ gas when a constant pressure of $2 \mathrm{atm}$ is maintained.

The value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction ${\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3+{\mathrm{Cl}}_2$ is $1.78$ at $250°\mathrm{C}$. The fraction of dissociation is $\mathrm{a} \times {10}^{-4}$ at equilibrium when $0.40$ mole of ${\mathrm{PCl}}_5$ is vaporised in a vessel containing $0.20$ mole of ${\mathrm{Cl}}_2$ gas when the volume is kept constant at $4$ litres.

Calculate the value of $\mathrm{a}$.

A volume of a gas weighing $8 \mathrm{g}$ was allowed to expand at a constant temperature until the pressure of the gas reduced to one-half of its former value. It was found that $500 \mathrm{mL}$ of the gas weighed $1.25 \mathrm{g}$. What was the original volume of the gas in Liter?