shitchan

1. A sample of ideal gas at room temperature occupies a volume of 31.0 L at a pressure of 612 torr . If the pressure changes to 3060 torr , with no change in the temperature or moles of gas, what is the new volume, V2 ?

2. If the volume of the original sample in Part A (P1 = 612 torr , V1 = 31.0 L ) changes to 61.0 L , without a change in the temperature or moles of gas molecules, what is the new pressure, P2 ?

3. A sample of ideal gas is in a sealed container. The pressure of the gas is 785 torr , and the temperature is 2 ∘C . If the temperature changes to 86 ∘C with no change in volume or amount of gas, what is the new pressure, P2 , of the gas inside the container?

4. Using the same sample of gas (P1 = 785 torr , T1 = 2 ∘C ), we wish to change the pressure to 7850 torr with no accompanying change in volume or amount of gas. What temperature T2 , in Celsius, is needed to reach this pressure?

5. A sample of gas in a balloon has an initial temperature of 37 ∘C and a volume of 1.86×10³ L . If the temperature changes to 89 ∘C , and there is no change of pressure or amount of gas, what is the new volume, V2 , of the gas?

6. What Celsius temperature, T2 , is required to change the volume of the gas sample in Part A (T1 = 37 ∘C , V1 = 1.86×10³ L ) to a volume of 3.72×10³ L ? Assume no change in pressure or the amount of gas in the balloon.

Subject-civics

Writing Activity 16: "One Party, Two, or More"

Imagine that you are a political leader advising citizens on their country's future. In a one to two page essay, tell the citizens whether you think their country should have a one-party, two-party, or multiparty political system and why. You must explain the advantages and disadvantages for all party systems.
Consider:

• characteristics of a two-party system

• characteristics of a multiparty system

• advantages and disadvantages of a coalition government

For a certain amount of gas at constant temperature, the pressure and volume have an inverse relationship (Figure 1) . This is called Boyle's law:

P1V1=P2V2 A sample of ideal gas at room temperature occupies a volume of 32.0 L at a pressure of 692 torr . If the pressure changes to 3460 torr , with no change in the temperature or moles of gas, what is the new volume, V2 ? If the volume of the original sample in Part A (P1 = 692 torr , V1 = 32.0 L ) changes to 60.0 L , without a change in the temperature or moles of gas molecules, what is the new pressure, P2 ?

1.Does gas kinetic energies depend on absolute temperature? Yes/No

2. According to Boyle's Law, if the pressure applied to an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is halved. T/F

3. The Ideal Gas Law is best applied at low temperature and high pressure. T/F

3)Which of the following statements are correct?(Select all of the above that apply)

a. Two moles of chlorine gas at 20 °C is heated to 250 °C while the volume is kept constant. The density of the gas increases.

b. According to Boyle's Law; if the pressure applied to an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is halved.

c. Under the same pressure and temperature; the volume of 2 mol of O22 gas is larger than that of 2 mol of N22 gas.

d. According to Charles's Law; if the temperature (in K) of an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is doubled.

e. According to Avogadro's Law; if 0.35 mol of an ideal gas sample has a volume of 7.84 L; the volume of 1.05 mole of the gas is 23.5 L at the same temperature and pressure.

a Two moles of chlorine gas at 20 °C is heated to 250 °C while the volume is kept constant. The density of the gas increases.
b According to Boyle's Law; if the pressure applied to an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is halved.
c Under the same pressure and temperature; the volume of 2 mol of O2 gas is larger than that of 2 mol of N2 gas.
d According to Charles's Law; if the temperature (in K) of an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is doubled.
e According to Avogadro's Law; if 0.35 mol of an ideal gas sample has a volume of 7.84 L; the volume of 1.05 mole of the gas is 23.5 L at the same temperature and pressure.

Teacher Doesn't Post an Answer Sheet, Plz Help!

16. Kinetic energy is the energy of motion and change. (A). True (B). False

17. If a sample of 0.50 moles of He occupies 4.2 L under certain conditions, what volume will 0.23 moles occupy under the same conditions?

18. What is the volume of 2.75 g of H2 gas at 4.75 atm and 315 K?

19. A 0.465 g sample of an unknown compound occupies 0.245 L at 298 K and 17.9 psi. What is the molar mass of the unknown compound?

20. A mixture of 5.00 g of He and 5.00 g of Ne have a total pressure of 2.50 atm. What is the partial pressure of He?

21. Calculate the root mean square velocity of hydrogen molecules at 22.00 °C. Urms = (3RT/M) 1/2 where R = 8.314 J/mol.K

22. One of the following equation/law is used to calculate the properties of a gas under non-ideal conditions. (A). Dalton's Law (B). Charles's Law (C). Boyle's Law (D). van der Waals equation (E). Avogadro's Law

23. The atmospheric pressure is 720. mmHg. What is the pressure in inches of Hg (in Hg)?

24. Which of the following gas samples has the greatest density at STP? (A). SF6 (B). NO (C). He (D). CO2 (E). All of these materials have the same density at STP.

25. A mixture of 0.152 moles of NO, 0.245 moles of H2 and 0.993 moles of Ar has a total pressure of 5.75 atm. Calculate the partial pressure of Ar?

26. Calcium hydride (CaH2) reacts with water to form hydrogen gas, according to the following reaction. CaH2(s) + 2H2O(l) ïƒ Ca(OH)2(aq) + 2H2(g) How many grams of calcium hydride (CaH2) are needed to generate 2.50 L of hydrogen gas at a pressure of 0.900 atm and a temperature of 38.20 °C?

27. Consider the following combustion reaction: C2H4(g) + O2 (g) ïƒ CO2(g) + H2O(g) (not balanced) Determine the number of liters of CO2 gas formed at STP when 2.45 grams of C2H4(g) is burned with excess oxygen gas.

28. Which of the following gas will have the greatest volume at STP (A). 2.5 g N2 (B). 2.5 g O2 (C). 2.5 g Ar (D). 2.5 g NO (E). 2.5 g CO2

29. The volume of a gas is proportional to number of moles of a gas at constant pressure and constant temperature is known as (A). Ideal Gas Law (B). Charles's Law (C). Avogadro's Law (D). Dalton's Law (E). Boyle's Law

30. If a sample of 1.25 moles of Ne occupies 2.6 L under certain conditions, what volume will 8.79 moles of Ne occupy under the same conditions?

31. How many grams of KCl(s) are produced from the decomposition of KClO3(s) which produces 125.0 mL of O2(g) at 34.5°C and 1.22 atm pressure?

1). How many liters of oxygen gas are needed to exactly reactwith 27.8 g of methane at 22.0 oC and 637.0 torr

CH₄(g) + 2 O₂(g) ? CO₂(g) + 2H₂O(l) (balanced)

3) A 0.5800 g sample of gas occupies 140. mL of volume at 22.4^oC and 0.68 m Hg. What is the molar mass of the gas?

4) Ammonium nitrate (MM=80.052) decomposes explosively uponheating according to the following equation:

NH₄NO₃ (s)? N₂ (g) +O₂ (g) + H₂O (g) (reactionnot balanced)
Calculate the total volume (in L) of gas (at 156.5 ^oCand 146.0 kPa) produced by the complete decomposition of 1.550 kgof ammonium nitrate

When heated to 350C at 0.950 atm, ammonium nitrate decomposes to produce nitrogen, water, and oxygen gases: 2NH4NO3(s) --> 2N2(g)+4H20(g)+O2(g). a.) How many liters of water vapor are produced when 21.7g of NH4NO3 decomposes?b.) How many grams of NH4NO3 are needed to produce 16.0L of oxygen?

When heated to 350 ?C at 0.950 atm, ammonium nitrate decomposes to produce nitrogen, water, and oxygen gases: 2NH4NO3(s)?2N2(g)+4H2O(g)+O2(g)

How many liters of water vapor are produced when 28.7 g of NH4NO3 decomposes?

• Show the set-up of your work. 

1. How many moles of H2O are produced when 10.0 mol of C3H8 are burned in excess oxygen?

2. Determine the mass of NaCl produced when 1.25 mol of sodium (Na) reacts with excess chlorine.

3. Ammonium nitrate (NH4NO3) produces N2O and H2O when it decomposes. Determine the mass of N2O produced from the decomposition of 25.0 g of NH4NO3

26. A graph called a demand curve can be used to illustrate therelationship between the price of compact disc players and thequantity of compact disc players demanded. If there is evidencethat buyers' income and the price of cassette tape players alsoinfluence the demand for compact disc players, then a movementalong the curve can be caused by a change in either the:
A) price of compact disc players or buyers' income.
B) price of cassette tape players or buyers' income.
C) quantity of compact disc players demanded or buyers'income.
D) price of compact disc players or the quantity of compact discplayers demanded.

27. A graph called a demand curve can be used to illustrate therelationship between the price of compact disc players and thequantity of compact disc players demanded. If there is evidencethat buyers' income and the price of cassette tape players alsoinfluence the demand for compact disc players, then a shift in thecurve can be caused by a change in either the:
A) price of compact disc players or buyers' income.
B) price of cassette tape players or buyers' income.
C) quantity of compact disc players demanded or buyers'income.
D) price of compact disc players or the quantity of compact discplayers demanded.

If A ⊂ Rn is a compact set and B ⊂ A, then B is a compact set?