The answer is 1. A sample of 0.50 moles of gas is placed in a container of volume of 2.5 L. What is the pressure of the gas in torr if the gas is at 25oC? P = 4.89 atm = 3719 torr
2. A sample of gas is placed in a container at 25oC and 2 atm of pressure. If the temperature is raised to 50oC, what is the new pressure? P = 2.17 atm
3. At 1 atm of pressure water boils at 100oC, if the sample was placed under 2 atm of pressure, what would be the temperature? (This would be like a pressure cooker).
T = 746 K = 473oC = 883oF
4. At what temperature would water boil if the pressure is 600 torr? (Use information from problem 3: this shows why food doesn't cook well at higher elevations)
T = 294 K = 21.5oC = 70.7oF
5. Calculate the volume of 40.6 g of F2 at STP. V = 23.9 L
6. A sample of 2.0 moles of hydrogen gas is placed in a container with a volume of 10.4 L. What is the pressure of the gas in torr if the gas is at 25oC? P = 4.70 atm = 3576
7. The tire pressure is 32 psi. What is the pressure in torr if 1 atm = 14.7 psi?
P = 1654 torr
8. A gas is placed in a balloon with a volume of 3.0 L at 28oC and 900 torr. What would be the new volume for the gas if placed under STP? V = 3.2 L
9. How many moles of gas would occupy a volume of 14 L at a pressure of 700 torr and a temperature of 30oC? n = 0.52 mol
10. Calculate the volume of 24.0 g of HCl at STP. V = 14.8 L
11. What is the volume of one mole of acetylene gas at STP? V =22.414 L
12. What is the volume of 0.75 mol of gas at 72oC and 2 atm? V = 10.6 L
13. After eating beans, a student collects a sample of gas at 0.97 atm and 26oC which occupies a volume of 3.5 L, calculate its volume at STP. V = 3.1 L
14. Ammonia (NH3) is placed in 1.5 L flask at 25oC. If the pressure of the gas is 0.899 atm, what is the density? d = 0.626 g/L
15. A mixture of Ar and CO gases is collected over water at 28oC and an atmospheric pressure of 1.05 atm. If the partial pressure of Ar is 600 torr, what is the partial pressure of CO? (vapor pressure of water at 28oC is 28.3 mmHg) PCO = 0.223 atm
16. Determine the partial pressures of each of the gases in the following mixture: 17.04 g NH3, 40.36 g Ne and 19.00 g F2. The gases are at 1.5 atm of pressure.
PNH3 = 0.428 atm; PNe = 0.857 atm; PF2 = 0.2124 atm
17. Potassium chlorate decomposes under heat as follows:
2 KClO3 (s) -------> 2 KCl (s) + 3 O2 (g)
The oxygen gas is collected over water at 25oC. The volume of gas is 560 mL measured at 1 atm. Calculate the number of grams of KClO3 used in the reaction. (vapor pressure of water = 0.0313 atm) nO2 = 0.022 mol; 1.81 g KClO3
Answer is: new substance.
For example, synthesis chemical reaction: Ba + F₂ → BaF₂.
Synthesis reaction is a type of reaction in which multiple reactants combine to form a single product.
New substance, barium fluoride is formed, with different chemical and ohysical properties than reactants (barium and fluorine).
In barium fluoride, barium has oxidation number +2 and fluorine has oxidation number -1, so compound has neutral charge.
The principle quantum number "n" represents the relative overall energy of each orbital, and the energy of each orbital increases as the distance from the nucleus increases. The sets of orbitals with the same "n" value are often referred to as electron shells or energy levels.
Answer:
The answer to your question is V2 = 1.82 l
Explanation:
Data
Volume 1 = 77 l
Pressure 1 = 18 mmHg
Volume 2 = ?
Pressure 2 = 760 mmHg
Process
Use Boyle's law to solve this problem
P1V1 = P2V2
-Solve for V2
V2 = P1V1/P2
-Substitution
V2 = (18 x 77) / 760
-Simplification
V2 = 1386 / 760
-Result
V2 = 1.82 l
Nonpolar covalent bonds are chemical bonds where two atoms share a pair of electrons with each other and the electronegativities of the two atoms are equal. An example is methane. It has four carbon-hydrogen single covalent bonds. These bonds are nonpolar because the electrons are shared equally.
