a. For the following unbalanced equation, calculate how many moles of the second reactant would be required to react completely with 0.608 grams of the first reactant. Al(s) + Br₂ (1)→ AlBr3 (8) mol Br₂ b. For the following unbalanced equation, calculate how many moles of the second reactant would be required to react completely with 0.956 grams of the first reactant. Hg(1) + HCIO4 (aq) → Hg(CIO4)2 (aq) + H₂(g) mol HC104 c. For the following unbalanced equation, calculate how many moles of the second reactant would be required to react completely with 0.692 grams of the first reactant. K(8) + P(8)→ K3P (8) mol P

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

For the following unbalanced chemical equation, suppose that exactly 2.00 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2 (g) + MnO2 (s) → Mn0(s) + H2 O(1) Limiting reactant: Mass of H20 = For each of the following unbalanced chemical equations, suppose that exactly 1.90 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICI is expected (assuming that the limiting reactant is completely consumed). I2 (s) + Cl2 (9) → ICI(9) Limiting reactant: Mass of ICl =

Consider the generic chemical equation: 2 A + 4 B --------> 3 C 1. If 10.0 moles of each reactant were used to complete that reaction, which of the following is true.  a. A is the limiting reactant and 15.0 moles of C will be produced. b. A is the limiting reactant and 20.0 moles of C will be produced. c. B is the limiting reactant and 7.50 moles of C will be produced. d. B is the limiting reactant and 22.5 moles of C will be produced.  2. What is the percent yield of this reaction if 6.40 moles of C were actually produced?

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

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

b For the following unbalanced chemical equation, suppose that exactly 6.10 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected (assuming that the limiting reactant is completely consumed). Enter the formula for the limiting reactant. MnO2 (s) + H2 SO4(ag) → Mn(SO4)2(s) + H2O(1) Limiting reactant: Mass of Mn(SO4)2 g Mass of H20 g

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