Question

Which of the following statements are true? A.The number of moles in 1.00 atm of gas was the same, despite the fact that the gases themselves had different identities. B.The number of moles in 1.00 atm of gas varied linearly with increasing molar mass. C.The volume of the gas varied depending on the identity of the gas. D.The number of moles in 1.00 atm of gas varied hyperbolically with increasing molar mass.

Given Avogadro's Law, which of the following statements are true? A.The number of molecules in a gas increases with temperature. B.The total number of atoms in a gas at STP can vary depending on the identity of the gas. C.The volume of a gas is independent of the pressure of the gas. D.The temperature of a gas is independent of the pressure of the gas.

In this experiment, the pressure of the gas was 1.00 atm and the temperature was 294.6 K. What value do you get for the gas constant using the data you recorded for propane? A.1.858 L atm mol-1 K-1 B.0.0008 L atm mol-1 K-1 C.0.0820 L atm mol-1 K-1 D.81.991 L atm mol-1 K-1

How many moles of methane were in the Erlenmeyer flask? A.1.72 × 10-3 mol B.6.23 × 10-3 mol C.6.23 × 10-2 mol D.2.26 × 10-3 mol

How many molecules of propane were in the Erlenmeyer flask? Avogadro's number is 6.022 × 1023 molecules/mol. A.6.022 × 1023 molecules B.3.74 × 1023 molecules C.7.50 × 1021 molecules D.3.74 × 1021 molecules

Suppose you have a mixture of ideal gases. Which of the following statements is false A.The gases will expand to fill the entire container. B.The total pressure is equal to the sum of partial pressures of the constituent gases. C.The mixture will behave as an ideal gas to a first approximation. D.The molar volume depends on the identity of the gases.

Answer #1

**1) Option A. The moles of an ideal gas do not depend on
your identity.**

**2) Option B. The total number of atoms depends on the
identity of the gas.**

**3) Option C. The correct value of the constants is 0.082
atm * L / mol * K**

**4) The moles are calculated:**

**n = P * V / R * T = 1 atm * 0.15 L / 0.082 atm * L / mol
* K * 294.6 K = 6.23x10 ^ -3 mol**

**5) Molecules are calculated:**

**molecules = n * NA = 6.23x10 ^ -3 * 6.02x10 ^ 23 =
3.74x10 ^ 21 molecules**

**Option D.**

**6) The false option is D. The molar volume does not
depend on the identity of the gases.**

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way, you would help me a lot, thank you.**

4. Three moles of a monatomic ideal gas are initially at a
pressure of 1.00 atm and a temperature of 20.0OC. The gas is
compressed adiabatically to a final pressure of 5.00 atm. Find: (a)
the initial volume of the gas; (b) the final volume of the gas; (c)
the final temperature of the gas; (d) the work done by the gas
during the compression.
Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8
atm-L
Please show...

For an ideal gas, calculate the following quantities.
(a) The pressure of the gas if 0.135 mol occupies 207 mL at
25°C.
______atm
(b) The temperature (in kelvins) at which 0.0250 mol occupies
1.00 L at 0.563 atm. K (c) The number of moles in 4.50 L at -7°C
and 715 torr. Remember 1atm = 760 torr.
_____mol
(d) The volume occupied by 4.72 10-3 mol at 40.°C and a pressure
of 1.57 kPa. Remember 1 atm = 101.325 kPa...

When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00
atm, H2O (l) and CO2 (g) are formed with the evolution of 50.33 kJ
of energy.
Substance
∆Hºf (kJ mol -1)
Sº (J mol -1 K -1)
H2O (l)
- 285.8
69.95
CO2 (g)
- 393.5
213.7
O2 (g)
0.0
205.0
C3H8 (g)
?
270.2
Calculate the molar enthalpy of combustion, ∆Hºcomb , of propane
and the standard molar enthalpy of formation, ∆Hºf , of propane
gas.

which of the following processes would cause the
volume of the gas sample to double?
a) the pressure applied to the gas is increased from
1.00 atm to 2.00 atm
b) the temperature of the sample is increased to 298k
to 596 k
c) the pressure applied to the gas is decreased from
4.00 atm to 1.00 atm
d) the number of moles of gas in the container is
halved

3. 10.0 moles of ideal gas cloud has an initial pressure of 1.00
bar, initial volume of 100.0L and temperature of 25.0ºC. The cloud
expands adiabatically to a final volume of 1000.0L. Cp,m= 20.79 J /
mol K (Cp,m is molar heat capacity and constant pressure)
a. (10 pts) What is the final pressure of the gas cloud?
b. (10 pts) What is the final temperature of the gas cloud?
c. (10 pts) What is the change in entropy for...

Rectangular PV Cycle
A piston contains 260 moles of an ideal monatomic gas that
initally has a pressure of 2.61 × 105 Pa and a volume of
4.9 m3. The piston is connected to a hot and cold
reservoir and the gas goes through the following quasi-static cycle
accepting energy from the hot reservoir and exhausting energy into
the cold reservoir.
1. The pressure of the gas is increased to 5.61 × 105
Pa while maintaining a constant volume.
2....

The ideal gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant Requals 0.08206 L⋅atm/(K⋅mol) or 8.3145
J/(K⋅mol). The equation can be rearranged as follows to solve for
n:
n=PVRT
This equation is useful when dealing with gaseous reactions
because stoichiometric calculations involve mole ratios.
A)When heated, calcium carbonate decomposes to yield calcium
oxide and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)
What is the mass of calcium carbonate...

a) A balloon is filled with 1000 liters of a gas on the ground
at 1.000 bar pressure and 25.6 oC temperature. What is
the number of moles of gas in the balloon? ( R= 0.08206 L.atm/mol.
K). 1 atm = 1.01325 bar.
b) If the balloon ascends to an altitude where the pressure is
0.620 bar and the temperature is 260 K, what is the molar mass of
the gas in the balloon if its densityis 0.8037 g/L?
c)...

1.00 g of 20Ne (molar mass 20.2 g/mol) in the gas phase is
contained inside a sealed cylinder with a piston that is free to
slide up and down. Initially, the gas is at atmospheric pressure
and occupies a volume of 1500 cm3 (state 1). The temperature of the
gas then increases to 500 K (state 2). Next, a rod is inserted
which holds the piston fixed in place, and the gas cools to a
temperature of 300 K (state...

± Stoichiometric Relationships with Gases
The ideal gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant Requals 0.08206 L⋅atm/(K⋅mol) or 8.3145
J/(K⋅mol). The equation can be rearranged as follows to solve for
n:
n=PVRT
This equation is useful when dealing with gaseous reactions because
stoichiometric calculations involve mole ratios.
Part A
When heated, calcium carbonate decomposes to yield calcium oxide
and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)...

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