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T₁ = 77°c=(77+273)K = 350k Gas Laws Worksheet -86°C = (86+273)K=359K Charles's Law (temperature, volume) 1) A 550.0 mL sample of nitrogen gas is warmed from 77 °C to 86 °C. Find its new volume if the pressure V₁ = √₂ remains constant. 564 ml T₁ V2= Vita (550.0 mL) x (359k) - √564 T₁ Ta m/

T₁ = 77°c=(77+273)K = 350k Gas Laws Worksheet -86°C = (86+273)K=359K Charles's Law (temperature, volume) 1) A 550.0 mL sample of nitrogen gas is warmed from 77 °C to 86 °C. Find its new volume if the pressure V₁ = √₂ remains constant. 564 ml T₁ V2= Vita (550.0 mL) x (359k) - √564 T₁ Ta m/

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Would you help me with the number 1 question? Also, can you show me the step-by-step and formula?
co 564 ml Charles's Law (temperature, volume) 1) A 550.0 mL sample of nitrogen gas is warmed from 77 °C to 86 °C. Find its new volume if the pressure remains constant. 2.22 L 350 k 2) A gas occupies 1.00 L at 0.00°C. What is the volume at 333.0 °C? V₁=1.00L 4₁ V₂ = V₁ = 1 V₂ = V₁Ta - (1.00 L) x (6061) - 2.222 273K 21300 L 26.6 L 318 K V₁=550.0 mL T₁ = 77°c = (77+273)k = 350k Gas Laws Worksheet -86°C -86+273)K=359K V₁ V₂ Boyle's Law (pressure, volume) 3) Convert 338 L at 63.0 atm to its new volume at 1.00 atm. P.V₁ Pala V2= Vita : (550.0 ML) x (359 k) T₁ 5730 mmHg Та .0313 atm T₁ T₂ -564mL +₁=0,00°C = 10.00+273) K=273k Ta333.0°C (333.0 +273 K = 606 K V₂= Pa 4) A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0 mm Hg. Find the volume of nitrogen when its pressure is changed to 400.0 torr while the temperature is held constant. P₁=63.0 atm V₁ = 3382 or 2.13 x 10 L = (63.0 atm) x (338L) = (2+13X10² L) Po=1.06A+m 7.00 atm 5) What pressure (mm Hg) is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters? Gay-Lussac's Law (temperature, pressure) 6) A gas has a pressure if 0.0370 atm at 50.0 °C. What is the pressure at 0.00 °C? k 7) If a gas in a closed container, with an original temperature of 25.0 °C, is pressurized from 15.0 atmospheres to 16.0 atmospheres, what would the final temperature of the gas be?
Transcribed Image Text:co 564 ml Charles's Law (temperature, volume) 1) A 550.0 mL sample of nitrogen gas is warmed from 77 °C to 86 °C. Find its new volume if the pressure remains constant. 2.22 L 350 k 2) A gas occupies 1.00 L at 0.00°C. What is the volume at 333.0 °C? V₁=1.00L 4₁ V₂ = V₁ = 1 V₂ = V₁Ta - (1.00 L) x (6061) - 2.222 273K 21300 L 26.6 L 318 K V₁=550.0 mL T₁ = 77°c = (77+273)k = 350k Gas Laws Worksheet -86°C -86+273)K=359K V₁ V₂ Boyle's Law (pressure, volume) 3) Convert 338 L at 63.0 atm to its new volume at 1.00 atm. P.V₁ Pala V2= Vita : (550.0 ML) x (359 k) T₁ 5730 mmHg Та .0313 atm T₁ T₂ -564mL +₁=0,00°C = 10.00+273) K=273k Ta333.0°C (333.0 +273 K = 606 K V₂= Pa 4) A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0 mm Hg. Find the volume of nitrogen when its pressure is changed to 400.0 torr while the temperature is held constant. P₁=63.0 atm V₁ = 3382 or 2.13 x 10 L = (63.0 atm) x (338L) = (2+13X10² L) Po=1.06A+m 7.00 atm 5) What pressure (mm Hg) is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters? Gay-Lussac's Law (temperature, pressure) 6) A gas has a pressure if 0.0370 atm at 50.0 °C. What is the pressure at 0.00 °C? k 7) If a gas in a closed container, with an original temperature of 25.0 °C, is pressurized from 15.0 atmospheres to 16.0 atmospheres, what would the final temperature of the gas be?
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