A student analyzes a hydrated coordination compound with the formula \(\text{K}_3[\text{Fe}(\text{C}_2\text{O}_4)_3]\cdot x\text{H}_2\text{O}\). During quantitative oxidation in excess \(\text{O}_2\), all the carbon atoms in the compound are converted to \(\text{CO}_2\), so each mole of the hydrate produces \(6\) moles of \(\text{CO}_2\). Heating a separate sample removes only the crystal water.

Analysis	Initial mass of hydrate	Other measured mass
Quantitative oxidation	\(0.491\text{ g}\)	\(0.264\text{ g of }\text{CO}_2\) collected
Dehydration	\(0.982\text{ g}\)	\(0.874\text{ g}\) of anhydrous residue

The molar masses of \(\text{CO}_2\) and \(\text{H}_2\text{O}\) are \(44.0\text{ g mol}^{-1}\) and \(18.0\text{ g mol}^{-1}\), respectively. Which pair gives the experimental average molar mass of the hydrate and the theoretical mass of crystal water in the dehydration sample, respectively?