Five grams of copper metal react with a solution containing twenty grams of silver nitrate to produce copper (II) nitrate and silver. a. What is the limiting reactant?
b. How much of the limiting reactant would be needed to react completely with the given amount of excess reactant?

a. AgNO₃ is limiting reactant

b. 26.7g of AgNO₃ would be needed

Explanation:

Based on the reaction:

Cu(s) + 2AgNO₃ → 2Ag(s) + Cu(NO₃)₂

1 mole of Cu reacts with 2 moles of AgNO₃

To find limiting reactant we need to convert mass of each reactant to moles using molar mass:

Moles Cu: Molar mass: 63.546g/mol:

5g * (1mol / 63.546g) = 0.0787moles of Cu

Moles AgNO₃: Molar mass: 169.87g/mol:

20g * (1mol / 169.87g) = 0.1177moles of AgNO₃

For a complete reaction of 0.0787moles of Cu are required:

0.0787moles Cu * (2 moles AgNO₃ / 1mol Cu) = 0.1574 moles AgNO₃

As there are just 0.1177 moles,

b. Would be needed 0.1574 moles of AgNO₃. In grams:

0.1574mol * (169.87g / mol) =

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.  

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be