Given the following reaction: \ce{cu + 2agno3 -> 2ag + cu(no3)2}cu+2agno3 2ag+cu(nox 3 )x 2 how many moles of \ce{ag}aga, g will be produced from 16.0 \text{ g}16.0 g16, point, 0, start text, space, g, end text of \ce{cu}cuc, u, assuming \ce{agno3}agno3 is available in excess

0.252 mol

Explanation:

Given the following reaction:

Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂

How many moles of Ag will be produced from 16.0 g Cu, assuming AgNO3 is available in excess.

First, we write the balanced equation.

Cu + 2 AgNO₃ → 2 Ag + Cu(NO₃)₂

We can establish the following relations.

The moles of Ag produced from 16.0 g of Cu are:

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

As the silver nitrate is in excess, the yielded moles of silver are computed from the 16g of copper as shown below, including the corresponding stoichiometric 1 to 2 relationship between copper and silver respectively:

Best regards.

"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."