As the magnesium reacts, the hydrogen gas produced is collected by water displacement at 23.0oC. The pressure of the gas in the collection tube is measured to be 749 torr. Given that the equilibrium vapor pressure of water is 21 torr at 23.0oC, calculate the pressure that the H2(g) produced in the reaction would have if it were dry.

The pressure that the produced in the reaction would have if it were dry will be 728 torr

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

Given :  =total pressure of gas = 749 torr

= partial pressure of hydrogen = ?

= partial pressure of water = 21 torr

putting in the values we get:

Thus the pressure that the produced in the reaction would have if it were dry will be 728 torr

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."