61. Consider the reaction between calcium oxide and carbon dioxide: CaO(s) + CO2(g) →→→→ CaCO3(s) A chemist allows 14.4 g of CaO and 13.8 g of CO₂ to react. When the reaction is finished, the chemist collects 19.4 g of CaCO3. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

2 g of aluminium metal is mixed with 11.5 g of sulphuric acid,H2SO4 to form aluminium sulphate and hydrogen gas. a)Write the balanced chemical equation for the reaction.

Consider the reaction. 2 Pb(s) + O₂(g) - 2 PbO (s) An excess of oxygen reacts with 451.4 g of lead, forming 361.0 g of lead(II) oxide. Calculate the percent yield of the reaction. percent yield:

Consider the following chemical equation: NH4NO3 (s) → N2O (g) + H2O (g) What would be the coefficients in front of each reactant and product in the balanced equation? If there would be no coefficient in front of a given compound in the balanced equation, just write type '1' NH4NO3 =? N2O =? H2O =?

of 15 An aqueous solution containing 9.88 g of lead(II) nitrate is added to an aqueous solution containing 5.48 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. balanced chemical equation: What is the limiting reactant? O lead(II) nitrate O potassium chloride The reaction goes to completion, but in the process of washing and drying the precipitate, some was lost. The percent yield for the reaction is 84.8%. How many grams of precipitate are recovered? F precipitate recovered: R V G Search or type URL % 5 T G B MacBook Pro 6 Y H & 7 N U J 8 00 M 1 ( 9 K O V H I ) O L P ^. { لا لا / 1 = ? 11 1 mi

What is the amount of excess reactant left over at the end of the reaction. Use the first image as an example.

Aqueous solutions barium chloride and potassium sulfate are combined.  1) Predict the products and write the balanced equation showing the states of each substance. 2) The barium chloride solution has a volume of 100.0 mL and contains 10.00 grams of barium chloride.  The molarity of the potassium sulfate solution is 0.574 moles/liter and has a volume of 100.0 mL. Determine the limiting reactant and the mass of each product in grams. 3) Determine how many grams of excess reactant remain. 4) Calculate the molarity of just the potassium ions after the reaction has finished.

For the following reaction: C3Hg(g) + O2(g) ————> CO2(g) + H2O(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams for each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams

Sodium hydroxide reacts with iron (III) chloride according to the following unbalanced chemical equation. What is the coefficient in front of the sodium chloride when the reaction is balanced? NaOH + Nacl FeCl3 Fe(OH)3 +

Classify each chemical reaction: Reaction Cl₂(g) + 2KI (aq) → 2KCl(aq) + 1₂ (s) H₂SO₂ (aq) H₂O(l) + SO₂ (g) PbCl₂ (aq) + FeSO (aq) → FeCl₂ (aq) + PbSO₂ (s) Mg(s) + F₂ (g) → MgF₂ (s) Type choose one choose one choose one choose one X Ś