a. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.255 mol of the first reactant. AgNO3(aq) + LiOH(aq) → AgOH(s) + LINO3(aq) g AgOH g LINO, b. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.155 mol of the first reactant. Al2(SO4)3 (aq) + 3CaCl₂ (aq) → 2AlCl3 (aq) + 3CaSO4 (8) g AlCl3 g CaSO4 c. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.215 mol of the first reactant. CaCO3 (8) + 2HCl(aq) → CaCl₂ (aq) + CO₂(g) + H₂O(1) g CaCl₂ g CO2 g H₂O

Consider the general chemical equation 3A+B→2C. Part A. If 1.45 g of A reacts with 1.75 g of B, what is the mass of C? Express your answer with the appropriate units. Part B. If 4.70 g of A reacts to produce 8.95 g of C, what is the mass of B? Express your answer with the appropriate units.

For the following reaction, 0.557 moles of potassium hydroxide are mixed with 0.224 moles of phosphoric acid. potassium hydroxide(aq)+phosphoric acid(aq)= potassium phosphate(aq)+water(l)   What is the formula for the limiting reagent? What is the maximum amount of potassium phosphate that can be produced?

Hydrogen fuel can be generated using a process called coal gasification. Hydrogen gas is formed by the reaction of carbon, excess oxygen and excess water.                         3C (from coal) + O2 + H2O → H2 + 3CO If this process has an 84.22% yield, what mass of coal (65.5%C by mass) is needed to generate 1.33 kg of hydrogen?

a. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.225 mol of the first reactant. Cl₂(g) + KI(aq) → 1₂ (s) + KCl(aq) mol KI b. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.405 mol of the first reactant. Co(s) + P4 (8)→ Co3 P2 (8) mol P4 c. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.415 mol of the first reactant. Zn(s) + HNO3(aq) → Zn(NO3)2 (aq) + H₂(g) mol HNO3 d. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.180 mol of the first reactant. C5 H12 (1) + O2(g) → CO2 (g) + H₂O(g) mol O2 abmit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous Next

3. What mass of NaCl can be produced from 0.55 mol Cl2 in the following reaction? 2 Naa + Cle) → 2 NaCle) d. 88 g a. 0.55 g b. 1.1 g с. 64 g С.

For the following reaction, 0.224 moles of sulfuric acid are mixed with 0.417 moles of calcium hydroxide. sulfuric acid (aq) + calcium hydroxide(s) → calcium sulfate(s) + water() What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of calcium sulfate that can be produced? Amount = moles

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + Mn0,(s) - MnCl, (aq) + 2 H,O(1) + Cl, (g) A sample of 41.7 g MnO, is added to a solution containing 49.7 g HCI. What is the limiting reactant? HCI O MnO2 What is the theoretical yield of Cl, ? theoretical yield: g Cl2 If the yield of the reaction is 84.3%, what is the actual yield of chlorine? actual yield: g Cl,

For the following reaction, 0.358 moles of sulfuric acid are mixed with 0.228 moles of zinc hydroxide. sulfuric acid(aq) + zinc hydroxide(s) → zinc sulfate(aq) + water(e) What is the formula for the limiting reagent? What is the maximum amount of zinc sulfate that can be produced? moles

According to the following reaction, how many grams of nitrogen monoxide will be formed upon the complete reaction of 24.6 grams of oxygen gas with excess nitrogen gas? N₂ (g) + O₂ (g) →→→2NO (g) grams nitrogen monoxide