Question

A 18.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.60 ✕ 105 Pa and temperature of 21.0°C. (a) Calculate the temperature of the gas in Kelvin. K (b) Use the ideal gas law to calculate the number of moles of gas in the tank. mol (c) Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole. g/mol (d) Obtain the number of grams of carbon dioxide in the tank. g (e) A fire breaks out, raising the ambient temperature by 224.0 K while 82.0 g of gas leak out of the tank. Calculate the new temperature and the number of moles of gas remaining in the tank. temperature K number of moles mol (f) Using the ideal gas law, find a symbolic expression for the final pressure, neglecting the change in volume of the tank. (Use the following as necessary: ni, the initial number of moles; nf, the final number of moles; Ti, the initial temperature; Tf, the final temperature; and Pi, the initial pressure.) Pf = (g) Calculate the final pressure in the tank as a result of the fire and leakage. Pa

Answer #1

A 22.0-L tank of carbon dioxide gas (CO2) is at a
pressure of 9.90 ? 105 Pa and temperature of 18.0°C.
(a) Calculate the temperature of the gas in Kelvin.
_______ K
(b) Use the ideal gas law to calculate the number of moles of gas
in the tank.
mol
(c) Use the periodic table to compute the molecular weight of
carbon dioxide, expressing it in grams per mole.
______ g/mol
(d) Obtain the number of grams of carbon dioxide...

A Carbon dioxide fire extinguisher initially contains 5.5lbm of
CO2 gas. In “real life” the CO2 would not be
all gas, but for this problem assume that it is. The CO2
gas has an initial pressure of 860psia and initial temperature of
+72oF. Immediately after putting out a fire, it has a
final pressure of 100psia and a final temperature of
-30oF. Assume ideal gas law behavior.
a) Show that the specific gas constant for CO2 gas is
approximately R=1131ft∙lbf/(slug∙R)....

1/ The stopcock connecting a 3.15 L bulb
containing carbon dioxide gas at a pressure of
9.69 atm, and a 4.15 L bulb
containing xenon gas at a pressure of
2.59 atm, is opened and the gases are allowed to
mix. Assuming that the temperature remains constant, the final
pressure in the system is .... atm.
2/ A mixture of xenon and
hydrogen gases, at a total pressure of
647 mm Hg, contains 10.3 grams
ofxenon and 0.403 grams of...

A sealed 51 m3 tank is filled with 9000 moles of
ideal oxygen gas (diatomic) at an initial temperature of 270 K. The
gas is heated to a final temperature of 330 K. The atomic mass of
oxygen is 16.0 g/mol. The mass density of the oxygen gas, in SI
units, is closest to
11
4.2
5.6
2.8
7.1

A mixture of krypton and carbon
dioxide gases is maintained in a 7.78 L
flask at a pressure of 3.03 atm and a temperature
of 15 °C. If the gas mixture contains
64.1 grams of krypton, the number
of grams of carbon dioxide in the mixture is
________ g.

An ideal monatomic gas is contained in a vessel of constant
volume 0.330 m3. The initial temperature and pressure of the gas
are 300 K and 5.00 atm, respectively. The goal of this problem is
to find the temperature and pressure of the gas after 24.0 kJ of
thermal energy is supplied to the gas.
(a) Use the ideal gas law and initial conditions to calculate
the number of moles of gas in the vessel. Your response differs
from the...

A high-pressure gas cylinder contains 40.0 L of toxic gas at a
pressure of 1.16 ✕ 107 N/m2 and a temperature
of 19.0°C. Its valve leaks after the cylinder is dropped. The
cylinder is cooled to dry ice temperature (−78.5°C) to reduce the
leak rate and pressure so that it can be safely repaired.
(a)
What is the final pressure in the tank in pascals, assuming a
negligible amount of gas leaks while being cooled and that there is
no...

1) 362.11 g of O2 are contained in a 3.00 L high pressure tank
at a temperature of 186°C. What is the pressure of the gas in
torr?
2) A gas has a given volume. The moles of gas are doubled then
the pressure is 1/3 of the original pressure. After the pressure
change, the Kelvin temperature quadruples (increases 4 times of the
original Kelvin temperature). By how much has the volume changed?
Be specific (i.e. the volume is 1/3...

n this week's experiment you will determine the molar mass of
carbon dioxide by measuring the mass of an Erlenmeyer flask full of
the gas. The following calculations are intended to familiarize you
with the general procedure:
The mass of an empty Erlenmeyer flask and stopper was determined to
be 58.85 grams. When filled with distilled water,
the mass was 303.4 grams. The atmospheric pressure
was measured to be0.9385 atm, the room temperature
was 20.00oC. At this temperature, the
vapor...

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...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 8 minutes ago

asked 13 minutes ago

asked 13 minutes ago

asked 13 minutes ago

asked 13 minutes ago

asked 18 minutes ago

asked 26 minutes ago

asked 27 minutes ago

asked 30 minutes ago

asked 31 minutes ago

asked 41 minutes ago