Question: What mass of Mg is required to completely react with5.0 mL of 5.0 M HC

Question

Question: What mass of Mg is required to completely react with5.0 mL of 5.0 M HCl? The balanced reaction is: 2Mg +2HCl ---> H(2) + MgCl(2) I figured out part of the process: Converted mL to L = .005L Molar mass of HCl = 36.4 g/mol Moles of HCL = .025 Moles of .025 HCl = .91 grams
But how to figure out the grams of Mg? Question: What mass of Mg is required to completely react with5.0 mL of 5.0 M HCl? The balanced reaction is: 2Mg +2HCl ---> H(2) + MgCl(2) I figured out part of the process: Converted mL to L = .005L Molar mass of HCl = 36.4 g/mol Moles of HCL = .025 Moles of .025 HCl = .91 grams
But how to figure out the grams of Mg?

Explanation / Answer

Moles of HCl = molarity * volume
                     = 5.0 M * 0.005 L                      =0.025 mol 2Mg +2HCl ---> H(2) + MgCl2 We can see 2 moles of magnesium reacting with 2 moles ofHCl So moles of magnesium required = 0.025 mol Mass of magnesium = moles * atomic mass                               =0.025 mol * 24.30 g/mol                               =0.6075 g

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