Question

1. The Ideal Gas Law equation is PV=nRT. Define each variable and include the unit necessary for each variable in the equation.

2. What is the pressure in a vessel of 4.5g of O_{2} gas
that takes up a volume of 4.2 L and is at a temperature of 38.2
^{o}C? (Use R = 0.0821 L-atm/mol-K).

3. A vessel of N_{2} gas was originally at a pressure of
3.4 atm, a volume of 2.3 L, and had a temperature of
21.5^{o}C. If the temperature is changed to
31.5^{o}C and the volume is decreased to 1.8 L, what will
the new pressure of the vessel be?

4. Why does the Ideal Gas Law break down at high pressures and low temperatures?

Answer #1

Consider the Ideal Gas Law, which states that PV = nRT, where P
is the pressure, V is the volume, T is the temperature, and n is
the number of moles of a gas sample, and R is a constant. (a)
Assume a sample of 1 mole of a gas is in a expandable container
where temperature and pressure are allowed to vary. Solve this
equation for V = f(P,T).
(b) Determine ∂V/dP and interpret the result. In particular,
describe...

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...

± 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)...

PVT relationship is based on an ideal gas law where PV=nRT..but
it is highly unlikely for a substance to behave ideally..thus other
correlations has been introduced such as Van der Waals equation,
Cubic EOS and Virial EOS.
In less than 300 word discuss the assumption made for these
equation and on what cases they most likely to be used. (can relate
to HYSYS lab also)

This problem involves solving the ideal gas law. The first three
questions are tied to Problem 1, so refer back to the problem
statement for conditions. Using the ideal gas equation, calculate
the pressure of oxygen gas in a cylinder with a volume of 25.00 L.
The oxygen masses 4.362 kg and room temperature is at 22.5oC. How
many moles of oxygen are there?
2.Using the same values of volume, mass, and room temperature
from Problem 1, calculate the pressure...

Butane, C4H10, is a component of natural gas that is used as
fuel for cigarette lighters. The balanced equation of the complete
combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00
atm and 23 ∘C, what is the volume of carbon dioxide formed by the
combustion of 2.80 g of butane? what is the volume of CO2?The ideal
gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant R equals 0.08206...

As will be discussed in detail in Chapter 5, the
ideal-gas equation of state relates absolute pressure, P(atm); gas
volume, V(liters); number of moles of gas, n mol ; and absolute
temperature, T(K): PV 0:08206nT
(a) Convert the equation to one relating P psig , V
(ft3) , n (lb-mole) , and T (°F) .
(b) A 30.0 mole%CO and 70.0 mole%N2 gas mixture is
stored in a cylinder with a volume of 3.5ft^3 at a temperature of
85°F. The...

Using molar volume (stp) or the ideal gas law equation, determine
the molar mass , g/mole, of each of the fillowin g.
1- 12.5 g of a gas that has a volume of 2.25 L at stp M
=
2- 0.742 g of a gas that has a volume of 835 ml at 1.10 ATM
and 19 degrees C. M=

1. According to the ideal gas law (also called the general gas
equation), how does temperature affect the partial pressure of O2
in air?
2. How does temperature affect the partial pressure of O2 in
water?
3. How does pH affect the partial pressure of O2 in water?
4. Please give examples of animals that use cocurrent,
countercurrent, and cross-current gas exchange.

1. Read the Chapter on Chemical Equilibrium: In particular, read
the section on the Le Chatelier Principle, as it relates to the
effects of concentration, pressure/volume, and temperature on the
position of a chemical equilibrium. 2. Solve the following related
problems involving the equilibrium between dinitrogen tetroxide and
nitrogen dioxide. N2O4 <==> 2 NO2 The equilibrium constant
for this reaction is Kp = 0.60 at 350 degrees Kelvin. A 1.0 L
vessel contains the above two gases in equilibrium at...

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