If you could me solve ths is anyway, it would be much appreciated.
A solution containing 3.50g of sodium carbonate is mixed with one that contains 5.00g of
silver nitrate.
a. Write the complete chemical equation and the net ionic equation for the reaction that
occurs.
b. What mass of any reactant left and product formed are present when the reaction is
complete?
This is a busy work problem. Also, it is a limiting reagent problem.
2AgNO3(aq) + Na2CO3(aq) ==> Ag2CO3(s) + 2NaNO3(aq)
2Ag^+(aq) + CO3^2- ==> AgCO3(s)
mols AgNO3 = grams/molar mass = ?
mols Na2CO3 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols AgNO3 to mols Ag2CO3
Do the same and convert mols Na2CO3 to mols Ag2CO3.
It is likely that the two values will not agree which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent.
Now you can convert mols Ag2CO3 to grams. g = mols x molar mass.
The above gives you the procedure for obtaining mass Ag2CO3 formed.
Using the limiting reagent only, you can convert that to mols NaNO3 and convert that to grams.
Using the limiting reagent only, you can convert that to mols of the "other" reactant used and subtracting from the initial amount will give you the amount left after the reaction is complete.
Someone will check your answers if you post your work.
To solve this problem, we need to follow a step-by-step approach:
Step 1: Write the balanced chemical equation
To write the chemical equation, we first need to determine the formulas of the compounds involved. Sodium carbonate is Na2CO3, and silver nitrate is AgNO3. The balanced chemical equation for the reaction can be written as:
2 AgNO3 + Na2CO3 → Ag2CO3 + 2 NaNO3
Step 2: Write the net ionic equation
The net ionic equation shows only the species that undergo a change during the reaction. To write the net ionic equation, we need to identify the soluble species and dissociate them into their respective ions. In this case, both sodium nitrate (NaNO3) and silver carbonate (Ag2CO3) are soluble ionic compounds. Thus, the net ionic equation can be written as:
2 Ag+ + CO3^2- → Ag2CO3
Step 3: Calculate the limiting reagent
The limiting reagent is the reactant that is completely consumed in a chemical reaction, limiting the amount of the product that can be formed. To determine the limiting reagent, we compare the number of moles of each reactant.
Given the mass of sodium carbonate as 3.50g and the molar mass of Na2CO3 as 106 g/mol, we can calculate the number of moles of sodium carbonate:
moles of Na2CO3 = mass / molar mass = 3.50g / 106 g/mol
Similarly, given the mass of silver nitrate as 5.00g and the molar mass of AgNO3 as 169.87 g/mol, we can calculate the number of moles of silver nitrate:
moles of AgNO3 = mass / molar mass = 5.00g / 169.87 g/mol
By comparing the moles of both reactants, we can determine which one is the limiting reagent.
Step 4: Calculate the amount of reactant left and the product formed
Based on the stoichiometry of the balanced chemical equation, we can calculate the amount of reactant left and the product formed once we know the limiting reagent.
For example, if sodium carbonate is the limiting reagent, then we can determine the moles of silver nitrate that reacted using the stoichiometric ratio of the balanced chemical equation.
Similarly, if silver nitrate is the limiting reagent, we can determine the moles of sodium carbonate that reacted.
To find the mass of any reactant left, subtract the moles reacted from the initial moles and then multiply by the molar mass of the respective compound.
To find the mass of the product formed, multiply the moles of the product by its molar mass.
I hope this explanation helps you solve the problem. If you have any further questions, feel free to ask!