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calculate mL of 6.0 M HCl required to react with 200 mL of .50 M KMnO4?I know the answer is 13.0 mL but I keep getting the wrong answer. I know im doing the first part right just not the last part200 ml KMnO4 x (.50 mol KMnO4/1000 mL KMnO4) = .1 mol KMnO4 .1 mol KMnO4 x (8HCl/1 KMnO4) = .0125 mol HCland then I dont know what to do?Also will you help me do this I have my final tomorrow and I know this is going to be on the test!!!(using the same balanced equation) calculate L of Cl2 gas at stp produced by the reaction of 75.0 mL of 6.0 M HClI know the answer is 15 L I just want to know the steps to get there becuase I will need this for my test and I cant google it tomorrow!
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