How Many Grams of N2 are Required to Produce 100.0 l of NH3 at STP

Stoichiometry - Moles, Mass, Molecules and Volume Name: 1. 4 NH₃(g) + 5 O₂(g) → 6 H₂O(g) + 4 NO(g) a) What mass of NO(g) is produced when 2.00 mol of NH₃(g) are reacted with excess O₂(g)? Answer: ``` 2.00 mol NH₃ × 4 mol NO / 4 mol NH₃ × 30.01 g NO / 1 mol NO = 60.0 g NO ``` b) What mass of H₂O(g) is produced when 4.00 mol of O₂(g) are reacted with excess NH₃(g)? Answer: ``` 4.00 mol O₂ × 6 mol H₂O / 5 mol O₂ × 18.02 g H₂O / 1 mol H₂O = 86.5 g H₂O ``` c) What volume of NH₃(g) at STP is required to react with 3.00 mol of O₂? Answer: ``` 3.00 mol O₂ × 4 mol NH₃ / 5 mol O₂ × 22.4 L NH₃ / 1 mol NH₃ = 53.8 L NH₃ ``` d) What volume of NH₃(g) at STP is required to react with 0.750 mol of H₂O? Answer: ``` 0.750 mol H₂O × 4 mol NH₃ / 6 mol H₂O × 22.4 L NH₃ / 1 mol NH₃ = 11.2 L NH₃ ``` 2. C₅H₁₂(l) + 8 O₂(g) → 5 CO₂(g) + 6 H₂O(l) a) What mass of CO₂(g) is produced when 100.0 g of C₅H₁₂(l) is burned? Answer: ``` 100.0 g C₅H₁₂ × 1 mol C₅H₁₂ / 72.17 g C₅H₁₂ × 5 mol CO₂ / 1 mol C₅H₁₂ × 44.01 g CO₂ / 1 mol CO₂ = 304.9 g CO₂ ``` b) What mass of O₂(g) is required to produce 60.0 g of H₂O(l)? Answer: ``` 60.0 g H₂O × 1 mol H₂O / 18.02 g H₂O × 8 mol O₂ / 6 mol H₂O × 32.00 g O₂ / 1 mol O₂ = 142 g O₂ ``` c) What mass of C₅H₁₂(l) is required to produce 90.0 g of CO₂(g) at STP? Answer: ``` 90.0 g CO₂ × 1 mol CO₂ / 44.01 g CO₂ × 1 mol C₅H₁₂ / 5 mol CO₂ × 72.17 g C₅H₁₂ / 1 mol C₅H₁₂ = 29.5 g C₅H₁₂ ``` d) What volume of O₂(g) at STP is required to produce 70.0 g of CO₂(g)? Answer: ``` 70.0 g CO₂ × 1 mol CO₂ / 44.01 g CO₂ × 8 mol O₂ / 5 mol CO₂ × 22.4 L O₂ / 1 mol O₂ = 57.0 L O₂ ``` e) What volume of O₂(g) at STP is required to produce 48.0 L of CO₂(g) at STP? Answer: ``` 48.0 L CO₂ × 8 mol O₂ / 5 mol CO₂ = 76.8 L O₂ f) What mass of H₂O is made when the burning of C₅H₁₂ gives 106 L of CO₂ at STP? 106 L CO₂ × 1 mol CO₂ / 22.4 L CO₂ × 6 mol H₂O / 5 mol CO₂ × 18.02 g H₂O / 1 mol H₂O = 102 g H₂O 3. Tetraethyl lead, Pb(C₂H₅)₄, is an "antiknock" ingredient which was added to some gasoline. Tetraethyl lead burns according to this equation: 2 Pb(C₂H₅)₄(l) + 27 O₂(g) → 2 PbO(s) + 16 CO₂(g) + 20 H₂O(g) a) What volume of O₂(g) at STP is consumed when 100.0 g of PbO(s) are formed? 100.0 g PbO × 1 mol PbO / 223.2 g PbO × 27 mol O₂ / 2 mol PbO × 22.4 L O₂ / 1 mol O₂ = 135.5 L O₂ b) How many molecules of CO₂ are formed when 1.00 × 10⁻⁶ g of tetraethyl lead are burned? 1.00 × 10⁻⁶ g Pb(C₂H₅)₄ × 1 mol Pb(C₂H₅)₄ / 323.2 g Pb(C₂H₅)₄ × 16 mol CO₂ / 2 mol Pb(C₂H₅)₄ × 6.022 × 10²³ molecules CO₂ / 1 mol CO₂ = 1.49 × 10¹⁶ molecules CO₂ c) How many molecules of H₂O are formed when 135 molecules of O₂ react? 135 molecules O₂ × 20 mol H₂O / 27 mol O₂ × 6.022 × 10²³ molecules H₂O / 1 mol H₂O = 1.00 × 10²³ molecules H₂O d) What volume of O₂(g) at STP, in mL, is required to react with 1.00 × 10¹⁵ molecules of tetraethyl lead? 1.00 × 10¹⁵ molecules Pb(C₂H₅)₄ × 1 mol Pb(C₂H₅)₄ / 6.022 × 10²³ molecules Pb(C₂H₅)₄ × 27 mol O₂ / 2 mol Pb(C₂H₅)₄ × 22.4 L O₂ / 1 mol O₂ = 5.02 × 10⁻⁷ L O₂ = 5.02 × 10⁻⁴ mL O₂ 4. Nitromethane, a dragster fuel, burns according to the following reaction: 4 CH₃NO₂(l) + 3 O₂(g) → 4 CO₂(g) + 6 H₂O(g) + 2 N₂(g) a) What mass of H₂O is produced when 0.150 g of CH₃NO₂(l) is burned? 0.150 g CH₃NO₂ × 1 mol CH₃NO₂ / 61.05 g CH₃NO₂ × 6 mol H₂O / 4 mol CH₃NO₂ × 18.02 g H₂O / 1 mol H₂O = 0.0664 g H₂O b) What combined volume of gas at STP is produced if 0.316 g of CH₃NO₂(l) is burned? 0.316 g CH₃NO₂ × 1 mol CH₃NO₂ / 61.05 g CH₃NO₂ × 12 mol gas / 4 mol CH₃NO₂ × 22.4 L gas / 1 mol gas = 0.348 L gas c) What volume of O₂(g) at STP is required to produce 0.250 g of CO₂(g)? 0.250 g CO₂ × 1 mol CO₂ / 44.01 g CO₂ × 3 mol O₂ / 4 mol CO₂ × 22.4 L O₂ / 1 mol O₂ = 0.0954 L O₂ d) What mass of H₂O(g) is produced when 0.410 g of CO₂ is produced? 0.410 g CO₂ × 1 mol CO₂ / 44.01 g CO₂ × 6 mol H₂O / 4 mol CO₂ × 18.02 g H₂O / 1 mol H₂O = 0.252 g H₂O 5. A sample of high purity silicon is prepared by strongly heating hydrogen and silicon tetrachloride in a sealed tube. SiCl₄(g) + 2 H₂(g) → Si(s) + 4 HCl(g) If exactly 1.00 g of silicon is required, what mass of each of SiCl₄(g) and H₂(g) must react? 1.00 g Si × 1 mol Si / 28.09 g Si × 1 mol SiCl₄ / 1 mol Si × 169.89 g SiCl₄ / 1 mol SiCl₄ = 6.05 g SiCl₄ 1.00 g Si × 1 mol Si / 28.09 g Si × 2 mol H₂ / 1 mol Si × 2.02 g H₂ / 1 mol H₂ = 0.144 g H₂ 6. Hydrazine, N₂H₄, is a rocket fuel which is prepared according to the reaction: 2 NH₃(g) + NaOCl(aq) → N₂H₄(l) + NaCl(aq) + H₂O(l) NaOCl is common "bleach" and NH₃(g) is prepared by passing NH₃(g) into water. If 1.25 × 10⁴ kg of hydrazine is required, how many liters of ammonia gas, at STP, is required in the reaction? 1.25 × 10⁴ kg N₂H₄ × 1000 g N₂H₄ / 1 kg N₂H₄ × 1 mol N₂H₄ / 32.05 g N₂H₄ × 2 mol NH₃ / 1 mol N₂H₄ × 22.4 L NH₃ / 1 mol NH₃ = 1.75 × 10⁷ L NH₃ 7. One of the most efficient drying agents known as P₄O₁₀ will even remove water from pure H₂SO₄ to produce SO₃ in the manner shown: P₄O₁₀(s) + 6 H₂SO₄(l) → 4 H₃PO₄(aq) + 6 SO₃(g) Pure H₂SO₄(l) has a density of 1.84 g/mL. If 25.0 mL of H₂SO₄(l) react, what mass of P₄O₁₀ also reacts and what volume of SO₃(g) at STP is produced? 25.0 mL H₂SO₄ × 1.84 g H₂SO₄ / 1 mL H₂SO₄ × 1 mol H₂SO₄ / 98.09 g H₂SO₄ × 1 mol P₄O₁₀ / 6 mol H₂SO₄ × 283.89 g P₄O₁₀ / 1 mol P₄O₁₀ = 10.5 g P₄O₁₀ 25.0 mL H₂SO₄ × 1.84 g H₂SO₄ / 1 mL H₂SO₄ × 1 mol H₂SO₄ / 98.09 g H₂SO₄ × 6 mol SO₃ / 6 mol H₂SO₄ × 22.4 L SO₃ / 1 mol SO₃ = 10.5 L SO₃