Question

A tank contains 12.3 g of chlorine gas (Cl_{2}) at a
temperature of 85 °C and an absolute pressure of 5.60 ×
10^{5} Pa. The mass per mole of Cl_{2} is 70.9
g/mol. **(a)** Determine the volume of the tank.
**(b)** Later, the temperature of the tank has dropped
to 27 °C and, due to a leak, the pressure has dropped to 3.10 ×
10^{5} Pa. How many grams of chlorine gas have leaked out
of the tank?

Answer #1

A rigid tank contains 65.5 g of chlorine gas (Cl2) at a
temperature of 73 °C and an absolute pressure of 5.60 × 105 Pa.
Later, the temperature of the tank has dropped to 33 °C and, due to
a leak, the pressure has dropped to 3.50 × 105 Pa. How many grams
of chlorine gas have leaked out of the tank? (The mass per mole of
Cl2 is 70.9 g/mol.) Answer in grams. Please provide a detailed
answer. Thank...

Q&A A tank contains 12.1 g of chlorine gas (Cl2) at a
temperature of 84 °C and an absolute pressure of 5.40 × 105 Pa. The
mass per mole of Cl2 is 70.9 g/mol. (a) Determine the volume of the
tank. (b) Later, the temperature of the tank has dropped to 29 °C
and, due to a leak, the pressure has dropped to 3.60 × 105 Pa. How
many grams of chlorine gas have leaked out of the tank?

Chapter 14, Problem 24 GO A tank contains 12.9 g of chlorine gas
(Cl2) at a temperature of 83 °C and an absolute pressure of 5.40 ×
105 Pa. The mass per mole of Cl2 is 70.9 g/mol. (a) Determine the
volume of the tank. (b) Later, the temperature of the tank has
dropped to 25 °C and, due to a leak, the pressure has dropped to
3.40 × 105 Pa. How many grams of chlorine gas have leaked out...

A steel tank contains 312 g of ammonia gs (NH3 with molar mass
17.0 g/mol) at a pressure of 1.43 x 106 and a temperature of
80.6oC. (a) What is the volume of the tank in liters? (b) Later the
temperature is 69.5oC and the pressure is 0.960 x 106 Pa. How many
grams of gas have leaked out of the tank? (Ignore the thermal
contraction of the tank.)

A welder using a tank of volume 7.30×10−2 m 3 fills it with
oxygen (with a molar mass of 32.0 g/mol ) at a gauge pressure of
3.15×105 Pa and temperature of 38.1 ∘ C . Remember that the guage
pressure of the gas in the tank is the difference between the
absolute pressure of the gas inside the tank and the pressure
outside the tank, in this case 1 atm. So the absolute pressure is
equal to the guage...

A welder using a tank
of volume 7.90×10−2 m3 fills it with oxygen (with a
molar mass of 32.0 g/mol ) at a gauge pressure of
3.30×105 Pa and temperature of 35.0 ∘C. Remember that
the guage pressure of the gas in the tank is the difference between
the absolute pressure of the gas inside the tank and the pressure
outside the tank, in this case 1 atm. So the absolute pressure is
equal to the guage pressure plus 1...

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...

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 17.0-L tank of carbon dioxide gas (CO2) is at a
pressure of 9.90 ✕ 105 Pa and temperature of 15.0°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...

Chlorine gas reacts with fluorine gas to form chlorine
trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.45 L reaction vessel,
initially at 298 K, contains chlorine gas at a partial pressure of
337 mmHg and fluorine gas at a partial pressure of 739 mmHg
.Identify the limiting reactant and determine the theoretical yield
of ClF3 in grams.

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