10. Ammonia reacts with copper(II) oxide according to the following equation: 2NH32 + 3CUO) → N + 3Cu + 3H;O@ a. When 62.00 g of ammonia is mixed with 350.0g CuO, which is the limiting reactant? b. What is the maximum mass in grams of copper that could be produced? c. How many grams of excess reactant are left over? d. If 245.8 g of copper is produced in this reaction, what is the percent yield?

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. In a neutralization reaction, 50.00 mL of 0.750 M phosphoric acid reacts with 2.500 g of magnesium hydroxide producing magnesium phosphate and water. Write a balanced equation for the reaction. b. What is the limiting reactant? C. How much of the excess reactant remains after the limiting reactant is completely consumed? d. What is the theoretical yield of magnesium phosphate (in grams)? e. If 2.552 g of magnesium phosphate are produced in an experiment, then what is the percent yield? a. lected

6. The gaseous hydrocarbon acetylene (C2H2) used in welders' torches, burns according to the following equation: 2C2H2(g) + 502(g)→ 4CO2(g) + 2H2O(g) a. What is the theoretical yield, in grams, of CO2, if 22.0 g of C2H2 completely reacts? b. If the actual yield in part a is 64.0 g of CO2, what is the percent yield of CO2 for the reaction?

Please do this, they are all parts of 1 question do all please.

Al2Cl6 is made by treating scrap metal with chlorine gas according to the following equation: 2 Al (s)   +   3 Cl2 (g)   ⟶⟶   Al2Cl6 (s)  In the reaction of 45.9 g Al with 212.5 g Cl2, determine the limiting reactant and theoretical yield of the product. The limiting reactant is? The theoretical yield of Al2Cl6 is?.  Round the answer to 1 decimal place. If the reaction produces 139.4 g Al2Cl6, calculate the percent yield of the reaction. ? %.     Round the answer to 1 decimal place.

a. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.642 mol of the first reactant were to react completely. CO₂(g) + 4H₂(g) → CH4 (9) + 2H₂O(1) mol CH4 mol H₂O b. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.622 mol of the first reactant were to react completely. BaCl₂ (aq) + 2AgNO3(aq) → 2AgCl(s) + Ba(NO3)2 (aq) mol AgCl mol Ba(NO3)2 c. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.618 mol of the first reactant were to react completely. C3H8 (g) + 5O2(g) → 4H₂O(1) + 3CO₂ (9) mol H₂O mol CO₂

Ammonia reacts with copper(II) oxide according to the following equation: 2NH3(g) + 3CuO(s) → N2(g) + 3Cu(s) + 3H2O(1) a. When 62.00 g of ammonia is mixed with 350.0g CuO, which is the limiting reactant? b. What is the maximum mass in grams of copper that could be produced? c. How many grams of excess reactant are left over? d. If 245.8 g of copper is produced in this reaction, what is the percent yield?

Balance the following reaction:__ Pb(NO3)2+ __ NaI → __ PbI2+ __ NaNO3 A) If 27 grams of lead (II) nitrate reacts with 17 grams of sodium iodide, how many grams of sodium nitrate can be formed? B)What is the limiting reactant? _________ The excess reactant? ___________ C) How many grams of the excess reactant will be left at the end of the reaction?

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 LINO3 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 AICI, 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(l) g CaCl2 g CO2 g H₂O Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous Next > Save and Exit