Sulfur dioxide reacts with liquid water to produce sulfurous acid SO2(g) + H2O -> H2SO3(aq) a. What is the percent yield if 18.07 g of sulfur dioxide reacts with excess water to produce 22.62 g of sulfurous acid? b. When 8.21 g of water reacts with sulfur dioxide, 26.79 g of sulfurous acid is produced. What is the percent yield?

What is the theoretical yield of HCI if 30.0 g of BCI3 and excess H20 are reacted according to the following balanced reaction? BC13(g) +3 H20(1) + H3BO3(s) + 3HCI(g) The following molar masses are: HCI = 36.46 g/mol BCI3 = 117.17 g/mol H2O = 18.02 g/mol

How many moles of H3PO4 are produced when 71 g of P4010 reacts completely P4010(s) + 6H20() → 4H3PO4(aq) O a 0.0635 moles H3PO4 O b 16.0 moles H3PO4 O c 4.00 moles H3PO4 O d 1.00 moles H3PO4

How much aspirin can be made from 100.0 g of salicylic acid and 100.0 g of acetic anhydride? If 122 grams of aspirin are obtained by the reaction, what is the percent yield?C7H6O3 + C4H6O3 arrow C9H8O4 + HC2H3O2 salicylic acid    acetic anhydride    aspirin     acetic acid

What is the theoretical yield of HCI if 30.0 g of BCI3 and excess H20 are reacted according to the following balanced reaction? BC13(g) +3 H20(1) H3BO3(s) + 3 HCI(g) The following molar masses are: HCI = 36.46 g/mol BCI3 = 117.17 g/mol %3D H20 = 18.02 g/mol 75.9 g HCI 132 g HCI 187 g HCI 56.0 g HCI 28.0 g HCI

A sample of 5.0 g of hydrogen gas reacts with 5.0 g of oxygen gas. 2H2 (g) + O2 (g) → 2H2O(l) d. How much excess reactant remains? e.If 4.2 g of water is actually produced, what is the percent yield?

1. Original volume of unknown NaCl solution = _______99.481______ mL   2. The concentration of Ag + within the 10 mL unknown NaCl solution after AgCl is added         [Ag+] = _______1.97412 x 10^(-10)_______________   3. Calculate the concentration of Cl- in the 10mL unknown NaCl solution. The Ksp for Silver Chloride is: 1.83 x 10-10.    Show your work below. AgCl(s)⇌Ag+(aq)+Cl−(aq)  Ksp=[Ag+][Cl−]       4. Calculate the mass of NaCl in the 10 mL unknown solution. Show your work. Hint:  mole = molarity x L; mass = mole x molar mass     5. Calculate the mass of NaCl in the original unknown solution. Show your work. mass of NaCl in the original unknown solution =             mass of NaCl in the 10 mL unknown solution x  ((?? ?? ???????? ?????? ?? ??????? ???? ????????) /10 ??)