How many grams of mgcl2 (molar mass = 95.20 g/mol) will be formed from 25.6 ml of a 0.100 m hcl solution reacting with excess magnesium metal? (the other product is hydrogen gas.)

0.1219 g

Explanation:

mole = mass/molar mass = molarity x volume

From the balanced equation of reaction:

1 mole of MgCl2 is formed from 2 moles of HCl

x mole of MgCl2 is formed from 0.1 x 0.0256 moles HCl

x mole of MgCl2 = 1 x 0.1 x 0.0256/2

                               = 0.00128

0.00128 moles of MgCl2 is formed from 0.00256 moles HCl

Hence,

mass of MgCl2 = moles x molar mass

                          = 0.00128 x 95.20

                            = 0.1219 g

Therefore, 0.1219 g of MgCl2 will be formed from 25.6 mL of a 0.100 M HCL solution reacting with excess magnesium metal.

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

increased stability in the completion of fluorine's outer shell.