(f) Si_(2)H_(6) reacts with oxygen. The equation for the reaction is: 2Si_(2)H_(6)(g)+7O_(2)(g)arrow 4SiO_(2)(s)+6H_(2)O(g) 30cm^3 of Si_(2)H_(6) is reacted with 150cm^3 (an excess) of oxygen. Calculate the total volume of gases present after the reaction. All volumes of gases are measured at the same temperature and pressure. __

## Step 1: Firstly, we need to understand the stoichiometry of the given balanced chemical equation. It states that for every 2 moles of silane ( ), 6 moles of water ( ) and 4 moles of silicon dioxide ( ) are produced. ## Step 2: Since the volume of gases is proportional to the number of moles at the same temperature and pressure (according to Avogadro's law), we can say that for every 2 volumes of silane, 6 volumes of water vapor are produced. ## Step 3: Given that we are reacting of silane, we can calculate the volume of water vapor produced by using the ratio derived from the balanced equation. ### ## Step 4: The total volume of gases after the reaction is the sum of the volume of the water vapor and the unreacted oxygen. ###