What is the mass of silver (107.87 g/mol) produced by the reaction of 3.00 moles of copper with 3.00 moles of silver nitrate?Cu + 2AgNO3→Cu(NO3)2+ 2Ag

323.61 g of will be produced

Explanation:

The given balanced chemical reaction is :

According to stoichiometry :

2 moles of require 1 mole of

Thus 3.00 moles of   will require=  of

Thus is the limiting reagent as it limits the formation of product.

As 2 moles of give =  2 moles of

Thus 3.00 moles of give =  of

Mass of

Thus 323.61 g of will be produced from the given moles of both reactants.

i don,t know so just answer mine

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol