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2= Boyle's Law (pressure, volume) PV=nr + >constant 3) Convert 338 L at 63.0 atm to its new volume at 1.00 atm. P.V₁ = Pay 21300 L P₁ V₁ Pa V₂ = 273K = 2.22L P₁ =63.0 atm V/2=2,13x10³2 V₁=3382 or 2.13 x 10 L (63.0 atm) x (338L) = (2.13X10¹L Pa = 1.06A+M

2= Boyle's Law (pressure, volume) PV=nr + >constant 3) Convert 338 L at 63.0 atm to its new volume at 1.00 atm. P.V₁ = Pay 21300 L P₁ V₁ Pa V₂ = 273K = 2.22L P₁ =63.0 atm V/2=2,13x10³2 V₁=3382 or 2.13 x 10 L (63.0 atm) x (338L) = (2.13X10¹L Pa = 1.06A+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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Can you help me with the number 3 question? Can you explain step by step including the formula (Boyle’s law)? I need to plug in the fraction to give the correct answer.
**Gas Laws Worksheet** **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.** - Formula: \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \) - Calculation: \( V_2 = \frac{(550.0 \text{ mL}) \times (359 \text{ K})}{350 \text{ K}} = 564 \text{ mL} \) **Answer: 564 mL** 2. **A gas occupies 1.00 L at 0.00°C. What is the volume at 333.0°C?** - Formula: \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \) - Calculation: \( V_2 = \frac{(1.00 \text{ L}) \times (606 \text{ K})}{273 \text{ K}} = 2.22 \text{ L} \) **Answer: 2.22 L** **Boyle’s Law (Pressure, Volume)** 3. **Convert 338 L at 63.0 atm to its new volume at 1.00 atm.** - Formula: \( P_1V_1 = P_2V_2 \) - Calculation: \( V_2 = \frac{(63.0 \text{ atm}) \times (338 \text{ L})}{1.00 \text{ atm}} = 21300 \text{ L} \) **Answer: 21300 L or \( 2.13 \times 10^4 \text{ L} \)** 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.** - Formula: \( P_1V_1 = P_2V_2 \) - Calculation: \( V_2 = \frac{(760.0 \text{ mmHg}) \times (14.0 \text{ L})}{400.0
Transcribed Image Text:**Gas Laws Worksheet** **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.** - Formula: \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \) - Calculation: \( V_2 = \frac{(550.0 \text{ mL}) \times (359 \text{ K})}{350 \text{ K}} = 564 \text{ mL} \) **Answer: 564 mL** 2. **A gas occupies 1.00 L at 0.00°C. What is the volume at 333.0°C?** - Formula: \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \) - Calculation: \( V_2 = \frac{(1.00 \text{ L}) \times (606 \text{ K})}{273 \text{ K}} = 2.22 \text{ L} \) **Answer: 2.22 L** **Boyle’s Law (Pressure, Volume)** 3. **Convert 338 L at 63.0 atm to its new volume at 1.00 atm.** - Formula: \( P_1V_1 = P_2V_2 \) - Calculation: \( V_2 = \frac{(63.0 \text{ atm}) \times (338 \text{ L})}{1.00 \text{ atm}} = 21300 \text{ L} \) **Answer: 21300 L or \( 2.13 \times 10^4 \text{ L} \)** 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.** - Formula: \( P_1V_1 = P_2V_2 \) - Calculation: \( V_2 = \frac{(760.0 \text{ mmHg}) \times (14.0 \text{ L})}{400.0
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