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Marti Andreski De La Salle HS

GASES. Marti Andreski De La Salle HS. How many liters of hydrogen and nitrogen are required to produce 30. L of ammonia gas at STP? (Qu. 27 on handout – part a). Step 1 – ID the problem type [ Volume – Volume at STP ] Step 2 – Write and balance the equation. N 2 + H 2  NH 3

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Marti Andreski De La Salle HS

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  1. GASES Marti Andreski De La Salle HS

  2. How many liters of hydrogen and nitrogen are required to produce 30. L of ammonia gas at STP? (Qu. 27 on handout – part a) • Step 1 – ID the problem type [Volume – Volume at STP] • Step 2 – Write and balance the equation. • N2 + H2 NH3 • Step 3 – Factor label to solve 3 2 1 mol NH3 3 mol N2 22.4 L N2 30.0 L NH3 = 45 L 2 mol NH3 22.4 L NH3 1 mol N2

  3. How many liters of hydrogen and nitrogen are required to produce 30. L of ammonia gas at STP? (Qu. 27 on handout – part b) • Step 1 – ID the problem type [Volume – Volume at STP] • Step 2 – Write and balance the equation. • N2 + H2 NH3 • Step 3 – Factor label to solve 3 2 1 mol NH3 1 mol H2 22.4 L H2 30.0 L NH3 = 15 L 2 mol NH3 22.4 L NH3 1 mol H2

  4. If 5.67 g of Mg reacts with HCl to form H2 at 99.7 kPa and 23.1oC, how much H2 forms? • Step 1 – ID: a mass to volume (non-std) • Step 2 – Write and balance the equation. • Mg + HCl  MgCl2 + H2 • Step 3 – Factor label to solve 2 1 mol Mg 1 mol H2 22.4 L N2 5.67 g Mg 1 mol Mg 24.1 g Mg 1 mol H2

  5. If 2.67 L of CH4 reacts with O2 to form CO2 and H2O at 99.7 kPa and 23.1oC, how much H2 forms? • Step 1 – ID: a mass to volume (non-std) • Step 2 – Write and balance the equation. • Mg + HCl  MgCl2 + H2 • Step 3 – Factor label to solve 2 1 mol Mg 1 mol H2 22.4 L N2 5.67 g Mg 1 mol Mg 24.1 g Mg 1 mol H2

  6. If 25.2 L of O2 at 749 torr and 21.3oC reacts with methane at 727 torr and 25.1oC, what volume of CO2 can be produced at STP? • Step 1 – ID: a mass to volume (non-std) • Step 2 – Write and balance the equation. • O2 + CH4 CO2 + H2O • Step 3 – Factor label to solve 2 2 1 mol Mg 1 mol H2 22.4 L N2 5.67 g Mg 1 mol Mg 24.1 g Mg 1 mol H2

  7. When 14.5 g of S burns, what volume of SO2 forms at 25oC and 755 mm? (qu. 32 on handout) • Step 1 – ID: a Mass to Volume (Non-Std) • Step 2 – Write and balance the equation. • S + O2 SO2 • Step 3 – Factor label and VPT 1 mol S 22.4 L SO2 = 10.1 L SO2 14.5 g S 1 mol SO2 32.1 g S 1 mol S 1 mol SO2 10.1 L ? 760 mm 755 mm 273 K 298 K

  8. If 40.0 ml of H2 measured at 22oC and 738 mm pressure is to be prepared from Mg and HCl, what mass Mg is used? (qu. 33 on handout) • Step 1 – ID: a Volme to Mass (Non-Std) • Step 2 – Write and balance the equation. • Mg + HCl  MgCl2 + H2 • Step 3 – VPT then Factor Label 2 ? 0.0400 L 738 mm 760 mm = 10.1 L SO2 295 K 273 K 14.5 g S 1 mol SO2 22.4 L SO2 1 mol S 32.1 g S 1 mol SO2 1 mol S

  9. When 14.5 g of S burns, what volume of SO2 forms at 25oC and 755 mm?

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