Question

The system consists of reactants (10.5 g of butane gas and the stoichiometric amount of oxygen gas) placed in a diathermic cylinder sealed from the surroundings by a diathermic, freely moving, massless piston. The cylinder is placed in a huge water tank at 300.K. In the initial state, the system is in equilibrium with the surroundings at 300.K and 1.0 atm. As a result of the combustion between the reactants, the system reaches a final state that contains only carbon dioxide gas and liquid water (i.e. the combustion reaction is assumed to have reached completion). In the final state, the temperature is still 300.K and the pressure is still 1.0 atm. Hence, the process is isothermal and isobaric. The balanced combustion reaction is written as:

C4H10 *(g)* + 13/2 O2 *(g)*à4 CO2*(g)* + 5
H2O*(l)*

Calculate the expansion/compression work, w, the heat, q, the
change in energy, ΔRU, and the change in enthalpy, ΔRH, associated
with the combustion of **10.5 g of butane**. Hints:
Assume ideal gas behavior for butane, oxygen and carbon dioxide and
neglect the volume of water liquid in the calculations. Indicate
whether the combustion process is an expansion or a compression and
make sure the sign of the work is consistent with that
observation.

Answer #1

we know that cylinder is diathermic that's why we see that

W = RT*ln (v_{2}/v_{1}) so here in this case W=
RTln(V/V/2)+RTln(V/2V) which will be equal to RT(ln(2)-ln(2)) = 0
so here what we get that from first law of theremodynamics

Q= u +w so chnage in q = change in U + change in W that will be
equal to change in U more over as we know that from ideal gas
relationship pv = RT so u will also be zero as T_{1} =
T_{2} but there will be heat because of motion of cylinder
which will be calculated by using force balance F = mg/A +
F_{G}

Butane undergoes combustion when it reacts with oxygen to
produce carbon dioxide and water.
2C4H10(g)+13O2(g)⟶Δ8CO2(g)+10H2O(g)
Part A
What volume, in liters, of oxygen is needed to react with 54.9 g
of butane at 0.84 atm atm and 29 ∘C?
Express your answer with the appropriate units.

Gaseous butane (CH3(CH2)2 CH3) reacts with gaseous
oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous
water ( H2O). If 67.2 g of carbon dioxide is produced from the
reaction of 38.94 g of butane and 202.1 g of oxygen gas, Calculate
the percent yield of carbon dioxide. Be sure your answer has the
correct number of significant digits in it.

Gaseous butane reacts with gaseous oxygen gas to produce gaseous
carbon dioxide and gaseous water. If 3.79g of carbon dioxide is
produced from the reaction of 4.1g of butane and 8.3g of oxygen
gas, calculate the percent yield of carbon dioxide. Be sure your
answer has the correct number of significant digits in it.

Gaseous butane (CH3CH22CH3) reacts with gaseous oxygen gas (O2)
to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If
0.650g of water is produced from the reaction of 1.2g of butane and
3.0g of oxygen gas, calculate the percent yield of water. Be sure
your answer has the correct number of significant digits in it.

± 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)...

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...

A mixture of propane and butane is burned with pure oxygen. The
combustion products contain 46.7 mole% H2O. After all the water is
removed from the products, the residual gas contains 68.8 mole% CO2
and the balance O2
a. What is the mole percent of propane in the fuel? %
b. It now turns out that the fuel mixture may contain not only
propane and butane but also other hydrocarbons. The fuel does not
contain oxygen. However, the dry combustion...

A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has
a pressure of 0.5015 atm when placed in a sealed container. The
complete combustion of the mixture to carbon dioxide gas, CO2(g),
and water vapor, H2O(g), was achieved by adding exactly enough
oxygen gas, O2(g), to the container. The pressure of the product
mixture in the sealed container is 2.421 atm. Calculate the mole
fraction of methane in the initial mixture assuming the temperature
and volume remain constant. Xch4=

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...

When methane (CH4) burns, it reacts with oxygen gas to produce
carbon dioxide and water. The unbalanced equation for this reaction
is CH4(g)+2O2(g)→CO2(g)+2H2O.What mass of carbon dioxide is
produced from the complete combustion of 4.50×10−3 g of
methane?

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