Question
Heres a balanced equation:
Na2CO3(aq)+2AgNO3 (aq) --> 2NaNO3(aq)+Ag2CO3 (s)
From this equation, 10 mL of AgNO3 in this contains 34 grams of AgNO3. Calculate the grams of solid product, Ag2CO3.
Part 2:
10 mL of Na2CO3 in this experiment contains 21 grams of Na2CO3. Calculation that the grams of solid product, Ag2CO3, expected from this reaction.
(please show steps please, I need to understand how you got the answer, thanks)
Na2CO3(aq)+2AgNO3 (aq) --> 2NaNO3(aq)+Ag2CO3 (s)
From this equation, 10 mL of AgNO3 in this contains 34 grams of AgNO3. Calculate the grams of solid product, Ag2CO3.
Part 2:
10 mL of Na2CO3 in this experiment contains 21 grams of Na2CO3. Calculation that the grams of solid product, Ag2CO3, expected from this reaction.
(please show steps please, I need to understand how you got the answer, thanks)
Answers
DrBob222
mols Ag (part a) = g/molar mass = about 0.2 but you need to do it more accurately.
Using the coefficients in the balanced equation convert mols AgNO3 to mols Ag2CO3. That is 0.2 mol AgNO3 x (1 mol Ag2CO2/2 mols Ag_) = 0.2 x 1/2 = aboaut 0.1 mol.
g Ag2CO3 formed = mols x molar mass
b. Do the same and solve for mols (then grams) Ag2CO3.
If the question is asking for grams Ag2CO3 with 34g AgNO3 and 21g Na2CO3 it turns into a limiting reagent problem in which case the FEWER mols Ag2CO3 will be formed..
Using the coefficients in the balanced equation convert mols AgNO3 to mols Ag2CO3. That is 0.2 mol AgNO3 x (1 mol Ag2CO2/2 mols Ag_) = 0.2 x 1/2 = aboaut 0.1 mol.
g Ag2CO3 formed = mols x molar mass
b. Do the same and solve for mols (then grams) Ag2CO3.
If the question is asking for grams Ag2CO3 with 34g AgNO3 and 21g Na2CO3 it turns into a limiting reagent problem in which case the FEWER mols Ag2CO3 will be formed..