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) =

b i think it’s a water wheel turning in a stream

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.