Question

1.) Imagine that you have a 7.00 L gas tank and a 4.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 155 atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer with the appropriate units.

2.) Part 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 needed to produce 25.0 L of carbon dioxide at STP? Express your answer with the appropriate units. Part B 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 4.00 g of butane? Express your answer with the appropriate units. 3.) One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 301 K , but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,V,T). View Available Hint(s)

Answer #1

**1) In order for both gases to exit at the same time,
they must have the same pressure, that is 155 atm.**

**2) Part A: The moles of CO2 are calculated:**

**n CO2 = P * V / R * T = 1 atm * 25 L / 0.082 * 273 K =
1.12 mol**

**The mass of CaCO3 is calculated:**

**m CaCO3 = 1.12 mol CO2 * (1 mol CaCO3 / 1 mol CO2) *
(100 g CaCO3 / 1 mol) = 112 g**

**Part B: I) The moles of CO2 formed are
calculated:**

**n CO2 = 4 g butane * (1 mol / 58.12 g) * (8 mol CO2 / 2
mol butane) = 0.275 mol**

**The volume is calculated:**

**V = n * R * T / P = 0.275 * 0.082 * 296 K / 1 atm = 6.7
L**

**3) The final pressure is calculated:**

**P2 = P1 * T2 / T1 = 1 atm * 301 K / 273 K = 1.10
atm**

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

Imagine that you have a 5.00 L gas tank and a 4.00 L gas tank.
You need to fill one tank with oxygen and the other with acetylene
to use in conjunction with your welding torch. If you fill the
larger tank with oxygen to a pressure of 155 atm , to what pressure
should you fill the acetylene tank to ensure that you run out of
each gas at the same time? Assume ideal behavior for all gases.

Imagine that you have a 6.00 L gas tank and a 4.00 L gas tank.
You need to fill one tank with oxygen and the other with acetylene
to use in conjunction with your welding torch. If you fill the
larger tank with oxygen to a pressure of 155 atm , to what pressure
should you fill the acetylene tank to ensure that you run out of
each gas at the same time? Assume ideal behavior for all gases.

Imagine that you have a 7.00 L gas tank and a 3.00 L gas tank.
You need to fill one tank with oxygen and the other with acetylene
to use in conjunction with your welding torch. If you fill the
larger tank with oxygen to a pressure of 145 atm , to what pressure
should you fill the acetylene tank to ensure that you run out of
each gas at the same time? Assume ideal behavior for all gases.

± 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)...

Imagine that you have a 6.00 L gas tank and a 2.00 L gas tank.
You need to fill one tank with oxygen and the other with acetylene
to use in conjunction with your welding torch. If you fill the
larger tank with oxygen to a pressure of 115 atm , to what pressure
should you fill the acetylene tank to ensure that you run out of
each gas at the same time? Assume ideal behavior for all gases.

Imagine that you have a 5.00 L gas tank and a 3.50 L gas tank.
You need to fill one tank with oxygen and the other with acetylene
to use in conjunction with your welding torch. If you fill the
larger tank with oxygen to a pressure of 125 atm , to what pressure
should you fill the acetylene tank to ensure that you run out of
each gas at the same time? Assume ideal behavior for all gases.

if you imagine that you have a
6.00 L gas tank and a 4.50 L gas tank. You need to fill one tank
with oxygen and the other with acetylene to use in conjunction with
your welding torch. If you fill the larger tank with oxygen to a
pressure of 115 atm , to what pressure should you fill the
acetylene tank to ensure that you run out of each gas at the same
time? Assume ideal behavior for all...

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...

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 1.60 g of butane?
Express your answer with the appropriate units.
volume of CO2 =

Acetylene torches are used for welding. These torches use a
mixture of acetylene gas, C2H2, and oxygen gas, O2 to produce the
following combustion reaction: 2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)
Part A Imagine that you have a 6.50 L gas tank and a 3.00 L gas
tank. You need to fill one tank with oxygen and the other with
acetylene to use in conjunction with your welding torch. If you
fill the larger tank with oxygen to a pressure of 105 atm , to...

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