### Gas Laws in Action: Temperature and Volume Relationship**Problem Statement:**A student produced 347 mL of hydrogen gas at -37.5 °C and constant atmospheric pressure. At what temperature (°C) will this gas expand to a volume of 750 mL?**Solution Approach:**To solve this problem, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature (in Kelvin) when pressure is constant. **Charles's Law Formula:**\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]Where:- \( V_1 \) is the initial volume of the gas (347 mL),- \( T_1 \) is the initial temperature (in Kelvin),- \( V_2 \) is the final volume of the gas (750 mL),- \( T_2 \) is the final temperature (in Kelvin).**Converting Temperatures to Kelvin:**- Initial temperature \( T_1 \): \[ T_1 = -37.5 °C + 273.15 = 235.65 \text{ K} \] **Setting Up the Equation:**\[\frac{347}{235.65} = \frac{750}{T_2}\]**Solving for \( T_2 \):**\[T_2 = \frac{750 \times 235.65}{347}\]**Converting Back to Celsius:**After calculating \( T_2 \) in Kelvin, convert it back to Celsius by subtracting 273.15. **Graphical Explanation:**If a graph were provided, it would typically show the direct relationship between Temperature (x-axis) and Volume (y-axis). The line should ideally be straight, illustrating the linearity between the two variables as per Charles's Law. **Answer Box:**An input field for students to enter their calculated temperature in Celsius.By solving this equation, students will gain a deeper understanding of the direct proportionality between the volume and temperature of a gas under constant pressure.

Answered: Image /qna-images/answer/dcd50ccc-de21-45db-95f2-203dc410dbef.jpg

Answered: A student produced 347 mL of hydrogen…

A student produced 347 mL of hydrogen gas at -37.5 °C and constan temperature (°C) will this gas expand to a volume of 750 mL?

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...

See similar textbooks

Similar questions

A sample of neon gas at a pressure of 774 mm Hg and a temperature of 44 °C, occupies a volume of 11.2 liters. If the gas is cooled at constant pressure to a temperature of 22 °C, What will the volume of the gas sample be in liters?
pe AMaps [References] An aerosol can contains 480. mL of compressed gas at 5.40 atm. When all of the gas is sprayed into a large plastic bag, the bag inflates to a volume of 2.26 L. What is the pressure of gas in the plastic bag? Assume a constant temperature. Pressure = atm
A gaseous mixture is heated from 25.0°C to 100°C in an expandable container. If the initial volume of the mixture was 10.0 L, what will be the final volume? (Assume pressure remains constant)
Use the References to access important values If needed for this question. A sample of argon gas occupies a volume of 6.85 L at 55.0°C and 1.19 atm. If it is desired to increase the volume of the gas sample to 9.72 L, while increasing its pressure to 1.59 atm, the temperature of the gas sample at the new volume and pressure must be °C. Submit Answer Retry Entire Group 8 more group attempts remalning
A sample of hydrogen gas at a pressure of 953 mm Hg and a temperature of 24 degree celcius,occupies a volume of 10.3 liters.If the gas is cooled at constant pressure to a temperature of -22 degree celcius,the volume of the gas sample will be ____L.
References Use the References to access important values if needed for this question. The stopcock connecting a 1.00 L bulb containing xenon gas at a pressure of 454 mm Hg, and a 1.00 L bulb containing nitrogen gas at a pressure of 526 mm Hg, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, what is the final pressure in the system? mm Hg
A sample of helium gas occupies a volume of 9.12 L at 54.0°C and 0.640 atm. If it is desired to decrease the volume of the gas sample to 6.16 L, while increasing its pressure to 0.852 atm, the temperature of the gas sample at the new volume and pressure must be ]°C.
38. I A sample of carbon dioxide gas at a pressure of 0.55o att and a temperature of 21.2°C occupies a volume of 12.9 liters. If the gas is allowed to expand at constant temperature to a volume
A hot air balloon is filled with 1.47 x 10° L of an ideal gas on a cool morning (11 °C). The air is heated to 127 °C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. L volume:
which staement is not true? 1.) A scuba diver should be certain to ascen fast from the dive 2.)While scuba diving with compressed air, the partial pressure of inhaled oxygen increases with increasing depth 3.) Nitrogen narcosis, which may be experienced by scuba divers, results from a direct effect of high nitrogen pressure on the nervous system 4.) The sum of partial pressure of all gases in a gas mixture can never add up to more than the total pressure of gas mixture 5.) none of these
A sample of hydrogen gas at a pressure of 1.14 atm and a temperature of 26.4° C, occupies a volume of 15.3 L. If the gas is allowed to expand at constant temperature to a volume of 20.3 L, the pressure of the gas sample will be atm.
A sample of neon gas at a pressure of 972 mmHg and a temperature of 49 degrees Celsius, occupies a volume of 13.7 liters. If the S is heated at constant pressure to a temperature of 98 degrees c, what will the volume of the gas sample be in Liters .