Question

A sample of CaCO3(s) is introduced into a sealed container of volume 0.674 L and heated to 1000 K until equilibrium is reached. The Kp for the reaction CaCO3(s)⇌CaO(s)+CO2(g) is 3.9×10−2 at this temperature. Calculate the mass of CaO(s) that is present at equillibrium.

please show work

Answer #1

Firstly write done the all things mentioned in the question.

V= 0.674L

T =1000K

Kp = pressure CO2 = 3.9 x 10^^{-2}

R = gas constant = 0.08206

We know the Ideal gas law pV= nRT

hence n= pV/RT

moles CO2 = pV/RT = 3.9 x 10^-2 x 0.654 / 0.08206 x
1000=0.000311

The number of moles of CO2 = Number of moles of CaO ( stiochemetric coefficient from the given reaction. It is 1:1)

hence moles CaO =0.000311

we know that

number of moles = weight of sample / Equivalent weight

molar mass of CaO = 56.077g/mol

hence

mass of CaO= moles x Equvalent weight(molecular weight)

mass CaO = 0.000311 mol x 56.077 g/mol=0.0174 g

**Answer: mass of CaO = 0.0174 g**

When 0.100 mol of CaCO3(s) and 0.100 mol of CaO(s) are placed in
an evacuated, sealed 10.0−L container and heated to 385 K, PCO2 =
0.220 atm after equilibrium is established: CaCO3(s) ⇌ CaO(s) +
CO2(g) An additional 0.290 atm of CO2(g) is pumped in. What is the
total mass (in g) of CaCO3 after equilibrium is reestablished?

For the reaction below, Kp = 1.16 at 800.°C. CaCO3(s)
equilibrium reaction arrow CaO(s) + CO2(g) If a 25.0-g sample of
CaCO3 is put into a 13.3 L container and heated to 800°C, what
percentage by mass of the CaCO3 will react to reach
equilibrium?

When 0.0430 mol of HI is heated to 500 K in a 5.00 L sealed
container, the resulting equilibrium mixture contains 2.85 g of HI.
Calculate Kc and Kp for the following decomposition reaction. 2 HI
(g) H2 (g) + I2 (g)

4.430g mixture containing CaCO3 (s) is heated until
all CaCO3 (s) is decomposed completly.
CaCO3 (s) >>>> CaO (s) +
CO2 (g) (Molar mass: CaCO3= 100.0g/mol CaO=
56.1g/mol CO2= 44.0g/mol)
If the mass of the mixture remaining after heating is 3.580g,
calculate the percent CaCO3 in the mixture from
the mass loss of the sample.

When heated, calcium carbonate (calcite) decomposes to form
calcium oxide and carbon dioxide gas
CaCO3(s) <----> CaO(s) + CO2(g)
Using the data below, calculate the equilibrium partial pressure of
CO2(g) over a mixture of solid CaO and CaCO3 at 500 ◦C if ∆CP,m for
the reaction is independent of temperature over the temperature
range between 25 ◦C and 500 ◦C
...............................CaO(s)..........CO2(g)..............
CaCO3(s)
∆H◦ f (kJ/mol) .......−635.09 ......−393.51
............−1206.92
S◦ m (J / mol K) ......39.75 .........213.74
.................92.90
CP,m (J /...

Calcium carbonate decomposes at high temperatures to give
calcium oxide and carbon dioxide as shown below. CaCO3(s) CaO(s) +
CO2(g) The KP for this reaction is 1.16 at 800°C. A 5.00 L vessel
containing 10.0 g of CaCO3(s) was evacuated to remove the air,
sealed, and then heated to 800°C. Ignoring the volume occupied by
the solid, what will be the overall mass percent of carbon in the
solid once equilibrium is reached?
A) 5.36%
carbon by mass
B)...

A solid sample consisting of 0.5 kg CaCO3 (s) was heated to 835
C (degrees) when it decomposed into gas CO2 (g) and solid CaO (s).
The heating carried out in a container fitted with a piston that
was initially resting on the solid such that volume change is due
to a formation of the gas.
Calculate the work done during the decomposition at 0.9 atm.

At 650 K, the reaction MgCO3(s)⇌MgO(s)+CO2(g) has Kp=0.026. A
14.4 L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260
atm. The container is then compressed to a volume of 0.800 L .Find
the mass of MgCO3 that is formed.

At 650 K, the reaction MgCO3(s)⇌MgO(s)+CO2(g)
has Kp=0.026. A 14.5 L container at 650 K has 1.0 g of
MgO(s) and CO2 at P = 0.0260 atm. The container is then
compressed to a volume of 0.200 L .
Find the mass of MgCO3 that is formed.

Using the table provided below, what is the entropy change if
4.5 g of CaCO3(s) is placed in a container and allowed to
decompose to CaO(s) and CO2(g) according to the
following reaction?
CaCO3(s) ⇔ CaO(s) + CO2(g)
Substance
S°
(J/mol × K)
CaCO3(s)
92.88
CaO(s)
39.75
CO2(g)
213.6
in J/K
Note: Report your final answer to the correct number of
significant figures and include the sign (+/-).

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