I'm having trouble with another chem problemAluminum sulfide reacts w/water to form aluminum hydroxide and hydrogen sulfide. Write the balanced chemical equation for this reaction and find how many grams of aluminum hydroxide are obtained from 14.2 g of aluminum sulfide.I already found the balanced equation but I need help on finding how many grams of aluminum hydroxide are obtained from 14.2 g of aluminum sulfide. Can someone please explain how it's done?
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You use the given grams of Aluminum Sulfide, and use stoichiometry. First convert the Aluminum Sulfide from grams to moles [14.2g (1 mole of Aluminum Sulfide/total mass of Aluminum sulfide)]. Then, set up a mole ratio of Aluminum Sulfide to Aluminum Hydroxide (you do this by creating a ratio of the coefficients of both Aluminum Sulfide and Aluminum Hydroxide from your balanced equation; moles of Aluminum Hydroxide/miles of Aluminum Sulfide). And then finally convert back to grams (total mass of Aluminum Hydroxide/ 1 mole of Aluminum Hydroxide). In total, it should look like this: [14.2(1 mol Al Sulfide/mass of Al Sulfide)(mols of Al Hydroxide/mols of Al Sulfide)(mass of Al Hydroxide/1 mol of Al Hydroxide)]
