Determine the limiting reactant in the reaction. Calculate the amount in grams of CO2 from thew amount of the limiting reactant that you used in the reaction which is called the theoretical yield. The calculate the percent yeild of CO2 for the reaction. The balanced equation is: H3C6H5O7 (aq) + 3 NaHCO3 (aq) --> Na3C6H5O7 (aq) + 3 H2O (l) + 3 CO2 (g) Data from experiment: Measured Mass of NaHCO3 is 1.01 grams Measured Mass of H3C6H5O7 is 1.52 grams Measured Mass of CO2 is 0.49 grams Molar Mass Data: H3C6H5O7 = 192.14 g/mol NaHCO3 = 84.01 g/mol CO2 = 44.01 g/mol

what is the balance chemical equation, complete ionic equation, and net ionic equation for CuSO4(aq) + Zn (NO3)2 (aq)? what is the balance chemical equation, complete ionic equation, and net ionic equation for Na2 CO3 (aq) + CaCl2 (aq)? what is the balance chemical equation, complete ionic equation, and net ionic equation for CuSO4 (aq) + NH4 Cl (aq)?

Determine the maximum (theoretical) and actual yield of CaCO3, in grams, that can be produced from the precipitation reaction given 105.99 mol of Na2CO3.  Na2CO3 (aq) + CaCl2 ⋅2H2O → CaCO3 (s) + 2NaCl(aq) + 2H2O(aq)

Balance the following reaction. If a reactant or product is not present, put a zero (0) in the blank. H+(aq) + H2O(l) + ClO-13(aq) + e-1 <--> Cl-1(g) + H+(aq) + H2O(l)

Gold(III)hydroxide is used for electroplating gold onto other metals. It can be made by the following reaction (note the equation is unbalanced) KAuCl4(aq) + NaɔCO3(aq) + 3H,O(1) - Au(OH);(aq) + NaCl(aq) + KCI(aq) + CO2(g) To prepare a fresh supply of Au(OH), a chemist at an electroplating plant has mixed 20.00g of KAUC1, with 25.00g of Na CO3 (both dissolved im excess water) a. How many grams of NaCO: will b'required to react with KAUCI4? (only 3 decimal places) g of NanCO b. what is the maximum number of grams of Au(OH); than can be formed? (only 2 decimal places) Activate Windows g of Au(OH); 11:04 Links 20°C 23-Nov- ch Ipcert | Delete

How many moles of acid and base are needed to produce 2.50 moles in the following equation. 3 Mg(OH)2 (s) + 2H3PO4(aq)=>Mg3(PO4)2 (s) + 6 H2O (l)

For the balanced reaction     Mn2(SO4)5(aq) + 10LiOH(aq) --> 2Mn(OH)5(s) + 5Li2SO4(aq)how many grams of lithium sulfate are produced by this reaction if 148 g of manganese (V) hydroxide are also produced?

4. An old antacid commercial claimed that each tablet of their product could "neutralize 47 times its mass in stomach acid". The active ingredient in the antiacid tablet, NaAl(OH)₂CO3, reacts with HCl in stomach acid according to this balanced reaction: NaAl(OH)₂CO3 + 4 HCl →→ NaCl + AlCl³ + 3 H₂O + CO₂ How many moles of HCl can a 1.03 g of antiacid tablet neutralize if the tablet contains 0.246 g of the active ingredient? If stomach acid has a concentration of 0.14 M HCl, assuming the density of stomach acid to be similar to that of water (1.00 g/mL), what is the mass of stomach acid that the 1.03 g of antiacid tablet can neutralize? Does this number support the claim in the commercial?

25.0 mL of a 0.200 M solution of Ba(NO3)2 is mixed with 15.0 mL of a 0.300M solution of Na2SO4.  The balanced reaction equation is:   Ba(NO3)2(aq)  + Na2SO4(aq)   à  BaSO4(s)   +  2NaNO3(aq)   What mass of BaSO4 should be produced?

Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?