A 12.0 L helium tank is pressurized to 28.0 atm. When connected to this tank, a balloon will inflate because the pressure inside the tank is greater than the atmospheric pressure pushing on the outside of the balloon. Assuming the balloon could expand indefinitely and never burst, the pressure would eventually equalize causing the balloon to stop inflating. What would the volume of the balloon be when this happens?Assume atmospheric pressure is 1.00 atm. Also assume ideal behavior and constant temperature.Volume: [box for input] L

Helium is a noble gas and it is having duplet configuration Helium atomic number is 2 Helium mass…

helium tank is pressurized to 28.0 atm. When connected to this tank, a balloon will inflate be tank is greater than the atmospheric pressure pushing on the outside of the balloon. Assuming the lefinitely and never burst, the pressure would eventually equalize causing the balloon to stop inflatin the balloon be when this happens? sume atmospheric pressure is 1.00 atm. Also assume ideal behavior and constant temperature. lume: L

helium tank is pressurized to 28.0 atm. When connected to this tank, a balloon will inflate be tank is greater than the atmospheric pressure pushing on the outside of the balloon. Assuming the lefinitely and never burst, the pressure would eventually equalize causing the balloon to stop inflatin the balloon be when this happens? sume atmospheric pressure is 1.00 atm. Also assume ideal behavior and constant temperature. lume: L

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

References Use the References to access important values if n At constant temperature, 34.4 L of N, at 0.830 atm is compressed to 12.9 L. What is the final pressure of N,?
Which statement is a postulate of the kinetic molecular theory of gases? The pressure exerted by the gas is due to the gas particles sticking to the container walls. O The pressure exerted by the is due to the gas particles colliding with the container walls. gas The pressure exerted by the gas is due to repulsions between the gas particles.
Solve correctly please.
A sample of gas contains has a pressure of 3.09 atm at 303 K. What is the pressure of the sample in atmospheres if the temperature decreased to 120 K under constant moles and volume? Do not include units when entering your answer.
An ideal gas is is put in a rigid container at 1.58 atm and 23.4°C. If the temperature is raised to 53.5°C, what is the new pressure of gas in atm ? Do not put units in your answer. Report your answer to 2 decimal places.
9. By what factor will the volume change when a balloon rises to a height where the pressure is one third, the temperature is one half, and one half of the moles escape? Begin by writing ideal gas law. Solve for one variable. Then show the algebraic relationship.
Assume that the temperatures in container A and B are the same. Container Container A Pressure 0.14 atm 0.42 atm Volume 1.52 L ?? L Moles 0.06 mol 0.1 mol Based on the data provided above, what is the value of the volume (in L) in container B? Report your answer to three decimal places.
Two moles of an ideal gas are placed in a container of ridged container and the pressure increases. What must happen to the temperature? Explain.
If one atmosphere of pressure is equal to 760 torr, a pressure of 675 torr is equal to what value in atmospheres (atm)?
A 93.0 L sample of dry air cools from 163°C to 12°C. What is the final volume of the gas is thepressure is maintained at 3.15 atm
15) A sample of gas at STP occupies 1.12 L at STP and has a mass of 1.007g. Determine the molar mass of the gas and the identity of the gas. Use equation 6.11 on page 192 of your textbook.
Predict the enthalpy change for the reaction below using the thermochemical equations provided. 2 C2H2 + 5 O2 --> 4 CO2 + 2 H2O 4 C + 2 H2 --> 2 C2H2 Δ Hrxn = + 226.7 kJ/mol C + O2 --> CO2 Δ Hrxn = - 393.5 kJ/mol 2 H2 + O2 --> 2 H2O Δ Hrxn = - 571.6 kJ/mol Group of answer choices -2372 kJ/mol -1192 kJ/mol -1919 kJ/mol -738.4 kJ/mol