Even if you can help answer one that would be a great help!
1. How many liters of NO(g) are produced when 0.85L of 2.00M HNO3 solution is added to 216g according to the equation. Which reactant is the limiting reactant?
3 Ag + 4 HNO3 -> 3 AgNO3 + NO + 2 H2O3
2. Calculate the mass of water produced when 0.333L of 0.500M NaOH is added to 3.0g of acetic acid. The equation is:
NaOH + HC2H3O2 -> NaC2H3O2 + H2O
3. Calculate the number of grams AgCl formed when 0.200L of 0.200M AgNO3 is added to 75.0 grams of CaCl2. The equation:
2 AgNO3 + CaCl2 -> 2AgCl + Ca(NO3)2
It's better to post questions separately. We sometimes pass them up if there are too many to do at one sitting.
1. How many liters of NO(g) are produced when 0.85L of 2.00M HNO3 solution is added to 216g according to the equation. Which reactant is the limiting reactant?
3 Ag + 4 HNO3 -> 3 AgNO3 + NO + 2 H2O3
This is a limiting reagent problem; I know that because amounts are given for BOTH reactants.
mols HNO3 = M x L = ?
mols Ag = grams/atomic mass
Using the coefficients int the balanced equation, convert mols HNO3 to mols NO.
Do the same for mols Ag to mols NO.
It is likely the two values will not agree which means one of them is wrong. The correct value in limitng reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent (LR).
Now take the smaller value of mols and convert to L NO.
L = 22.4 L/mol x # mols = ?
2. Calculate the mass of water produced when 0.333L of 0.500M NaOH is added to 3.0g of acetic acid. The equation is:
NaOH + HC2H3O2 -> NaC2H3O2 + H2O
This is another LR problem. The only difference is that the end product is to convert mols to grams instead of volume as in the NO problem. Carry forward to mols of the product(H2O), then g = mols x molar mass.
#3 is another LR problem.
Post your work if you get stuck.