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Would you help me with the number 5 question? Also, can you show me the step-by-step and formula?

Would you help me with the number 5 question? Also, can you show me the step-by-step and formula?

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
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 5 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?
Expert Solution
Step 1

We have given initial and final volumes and  initial pressure of air.We are asked to determine the final pressure of the air whose volume is 26 litres. Here we will use Boyle's law.

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