Chemistry

This is an equilibrium problem where you need to track how much $\text{CaCO}_3$ decomposes and use the resulting gas pressures to find $K_P$. Start by converting the 35% unreacted into moles of each substance at equilibrium, then use the ideal gas law to find the partial pressure of $\text{CO}_2$ produced—that's your only gaseous product. Remember that $K_P$ depends only on gas-phase species, so $\text{CaO}$ and solid $\text{CaCO}_3$ don't appear in the expression.

This is an equilibrium problem where you need to track how much $\text{CaCO}_3$ decomposes and use the resulting gas pressures to find $K_P$. Start by converting the 35% unreacted into moles of each substance at equilibrium, then use the ideal gas law to find the partial pressure of $\text{CO}_2$ produced—that's your only gaseous product. Remember that $K_P$ depends only on gas-phase species, so $\text{CaO}$ and solid $\text{CaCO}_3$ don't appear in the expression.