Calcium oxide is used to remove the pollutant $S{O}_2$ from smokestack gases. The overall reaction is:

CaO$(s)+S{O}_2(g)+\frac{1}{2}{O}_2(g)CaS{O}_4(s)$

For this reaction, $K_p=2\mathrm{.}38{10}^{15}.$

$5$th attempt

Part $1(1$ point$)$

What is the partial pressure of $S{O}_2$ in equilibrium with air and solid CaO if $P_{O2}$ in air is $0\mathrm{.}21$atm $?$

Part $2(1$ point$)$

Consider a sample of gas that contains $500$ moles of smokestack gas. How many molecules of $S{O}_2$ are contained in this sample?

$x10$