89. For each of the following unbalanced chemical equations, suppose 25.0 g of each reactant is...
For each of the following unbalanced chemical equations, suppose 1.20 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). a. UO2 (s) + HF(aq) → UF4(aq) + H2O(l) Limiting reactant: Mass of UF4 = Mass of H20 = b. NaNO3(aq) + H2SO4 (aq) → Na2SO4 (aq) + HNO3(aq) Limiting reactant: Mass of Na2SO4 = Mass of HNO3 =
For each of the following unbalanced reactions, suppose exactly 1.48 g of each reactant is taken. Indicate which reactant is the limiting reagent. Calculate the mass of each product that is expected. (a) UO2(s) + HF(aq) → UF4(aq) + H2O(l) limiting reagent [_]UO2 [_]HF UF4 produced g H2O produced g (b) NaNO3(aq) + H2SO4(aq) → Na2SO4(aq) + HNO3(aq) limiting reagent [_] NaNO3 [_] H2SO4 Na2SO4 produced g HNO3 produced g (c) Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g)...
Limiting Reactant Calculations C6H1206(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g) Starting with 25.0 g C6H12O6 and 15.5 g 02, what is the theoretical yield of CO2 in grams? Calculation based upon C6H1206 Calculation based upon 02 What is the limiting reactant? What is the theoretical yield?
Work each of the following problems. SHOW ALL WORK TO RECEIVE ANY CREDIT (Hint: Make sure your chemical equations are balanced.) 1. When 18.0 g of O2 reacts with 25.0 g of CHSOH, what is the limiting reactant? What is the theoretical yield in grams of CO2? C2HsOH +O2 CO2 +H2On 2. What is the limiting reactant when 126 g of Ag reacts with 142 g of HNO,? What is the theoretical yield in grams of AgNO3? AgNO (a) +NO+H2O...
24. For each of the following unbalanced equations, calculate how many moles of the second reactant would be required to react completely with 0.557 grams of the first reactant. a. Al(s) Br2(l)-AlBr3(s) b. Hg(s) + HCIO4(a?) Hg(CIO4(aq) +H2(8) c. K(s) + P(s)-K,P(s) d. CH4(g) + Cl2(g)-CCl4(1)+HCI(g)
For each of the following unbalanced reactions, suppose exactly 1.33 g of each reactant is taken. Indicate which reactant is the limiting reagent. Calculate the mass of each product that is expected. (a) UO2(s) + HF(aq) → UF4(aq) + H20(1) limiting reagent UO2 HF 9 UF4 produced 40 1. 55 H20 produced 497 0.18 X 9 (b) NaNO3(aq) + H2SO4(aq) → Na2SO4(aq) + HNO3(aq) limiting reagent NaNO3 H2SO4 Na2SO4 produced 4.0) 1. 11 HNO3 produced 4. 0 0.99 9 X...
1. When 18.0g of O2 reacts with 25.0 g of C2H5OH, what is the limiting reactant? What is the theoretical yield in grams of CO2? C2HsOHo +O2(g) CO2 () H2O0
This question has multiple parts. Work all the parts to get the most points. a For the following unbalanced chemical equation, suppose that exactly 1.85 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS2() + O2(g) + CO2(g) + SO2(9) Limiting reactant Mass of CO2 = b For the following unbalanced chemical equation, suppose that exactly 1.40 g of each reactant...
C6H12O6(s) + 6 02(g) → 6 CO2(g) + 6 H2O(g) Starting with 25.0 g C6H12O6 and 15.5 g 02, what is the theoretical yield of CO2 in grams? Calculation based upon C6H1206 Calculation based upon 02 What is the limiting reactant? What is the theoretical yield?
For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of 14.2 g of the first reactant. (a) CO2(g) + H2(g) → CH4(9) + H20(1) CH4 4.9.) 14.2 x g H20 49 11.618 X Check the number of significant figures. g (b) TiBr4(9) + H2(g) → Ti(s) + HBr(9) Ti 4.9.169.9 X 9 HBr 4.9) 1011.37 x g (c) NaOH(s) + CO2(g) → Na2CO3(s) + H20(1) Na2CO3 407 H20 49...