- Tutor Answers
- Chemistry

Question

175155
What happens to the pressure of just the H2 gas in the flask after the introduction of the Ar?

Category:
Chemistry

Verified Textbook Solution:

A flask equipped with a valve contains 3.0 mol of H2 gas. You introduce 3.0 mol of Ar gas into the flask via the valve and then seal the flask. a. What happens to the pressure of just the H2 gas in the flask after the introduction of the Ar? If it changes, by what factor does it do so?

Coursepivot December 1, 2022 13:57

Explanation The pressure of the H2 in the flask will remain the same whether there is any other gas added or not. The pressure of a gas in the flask (View full solution)

Category:
Chemistry

Verified Textbook Solution:

Consider a sealed glass bottle of helium gas at room temperature. If you immerse the bottle in an ice water bath, how will this immersion affect the pressure of the gas? I. Pressure increase II. Pressure decrease III. No pressure change The best explanation for your answer is? a. The force of the co...

Coursepivot December 1, 2022 13:56

Explanation The fact that pressure decreases can be seen by observing the ideal gas law: PV = nRT Volume, moles and the gas constant are all constant, so reducing temperature (View full solution)

Category:
Chemistry

Verified Textbook Solution:

How many liters of chlorine gas, Cl2, can be obtained at 40°C and 787 mmHg from 9.41 g of hydrogen chloride, HCl, according to the following equation? 2KMnO4(s)+16HCl(aq)→8H2O(l)+2KCl(aq)+2MnCl2(aq)+5Cl2(g)

Coursepivot December 1, 2022 13:20

Explanation For this question, we shall be using the ideal gas law equation, PV = nRT. Where P is in atm, V in liters, R = 0.08206 L-at/ mol-K and (View full solution)

Category:
Chemistry

Verified Textbook Solution:

Calculate the density of helium, He, in grams per liter at 21°C and752 mmHg. The density of air under these conditions is 1.188 g/L. What is the difference in mass between 1 liter of air and 1 liter of helium? (This mass difference is equivalent to the buoyant, or lifting, force of helium per liter....

Coursepivot December 1, 2022 13:17

Explanation Assume you have exactly one mole of He; determine the mass and the volume independently, then divide to get density. You can figure out the mass in grams of (View full solution)

Category:
Chemistry

Verified Textbook Solution:

Three 3.0-L flasks, each at a pressure of 878 mmHg, are in a room. The flasks contain He, Ar, and Xe, respectively. a. Which of the flasks contains the most atoms of gas?

Coursepivot December 1, 2022 13:17

Explanation PV = nRT Since pressure, volume and temperature are same for all the gases ,hence the moles of all the gases will also be the same. Number of atoms (View full solution)