Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. if 10.6 grams of aluminum hydroxide is produced, how many grams of water were reacted?

There reacts 7.35 grams of H2O

Explanation:

Step 1: Data given

Mass of aluminium hydroxide = 10.6 grams

Step 2: The balanced equation

Al2S3(s) + 6H2O(l) → 2Al(OH)3(s) + 3H2S(g)

Step 3: Calculate number of moles Al(OH)3

Moles Al(OH)3 = mass Al(OH)3 / molar mass Al(OH)3

Moles Al(OH)3 = 10.6 grams / 78.00 g/mol

Moles Al(OH)3 = 0.136 moles

Step 4: Calculate moles of H2O

For 1 mol of Al2S3 we need 6 moles of H2O to produce 2 moles of Al(OH)3 and 3 moles of H2S

For 0.136 moles of Al(OH)3 we need 3*0.136 = 0.408 moles of H2O

Step 5: Calculate mass of H2O

Mass H2O = moles H2O * molar mass of H2O

Mass H2O = 0.408 * 18.02 = 7.35 grams

There reacts 7.35 grams of H2O

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.