Question

Question #59eb8

Answer 1

See below.

Explanation:

The reaction is `Fe_2O_3 + 3CO -> 2Fe + 3CO_2`.
And ,the molar masses(g/mol) for the substances are:
`Fe: 55.85`
`Fe_2O_3: 159.69`
`CO: 28.01`
`CO_2: 44.01`

Gas constant is
`R=8.314 (JK^-1mol^-1)`
`=0.08206 (LatmK^-1mol^-1)`

Temparature is `0℃=273.15K`.

Now we're ready to use the ideal gas law: `PV=nRT`.
The volume of gas is `V=(nRT)/P`.

[Upper row]
`1000` kg of `Fe_2O_3` is
`(1000*10^3) /159.69 = 6.262*10^3` mol.

Thus, `6.262*10^3 * 2 = 1.252*10^4` mol of `Fe` is obtained and its mass is `1.252*10^4*55.85=6.99*10^5` (g) `=699` (kg). This is right.

You need `6.262*10^3*3=1.879*10^4` mol of `CO` and its mass is `1.879*10^4*28.01=5.26*10^5` (g) `=526` (kg).

Obtained `CO_2` is also `1.879*10^4` mol and its volume is
`V=(1.879*10^4 * 0.08206 * 273.15)/1 =4.212*10^5 (L) =421.2(m^3)`.
`426.3(m^3)` in the table is a bit too large.

[Lower row]
`104.9` kg of `Fe` is `(104.9*10^3)/55.85 = 1.878*10^3` mol and to obtain this, you need `(1.878*10^3) /2 = 9.390*10^2` mol of `Fe_2O_3`. The mass of `Fe_2O_3` is `9.390*10^2*159.69=1.500 *10^5` (g) =`150.0` (kg).

The mass of `CO` is `228.9-150.0` = `78.9` (kg) and its amount of substance is `(78.9*10^3)/28.01=2.817*10^3` (mol). This is three times of that of `Fe`(`9.39*10^2` mol) and matches the chemical equation.

Obtained `CO_2` is also `2.817*10^3` mol. Its volume under `25℃,850` mmHg is
`V=(2.817*10^3*0.08206*(273.15+25))/(850/760)`
`=6.162*10^4` (L).

Answer 2

There are no "incorrect" values unless you require a "balanced" outcome, which rarely happens in practice.

Explanation:

The "filling in the blanks" can be done with the given data and the balanced chemical equation.
`Fe_2O_3 + 3CO -> 2Fe + 3CO_2`

Converting the mass to moles for iron and the volume to moles for the `CO_2` is needed in the first line.

Iron Oxide `1000/159.7 = 6.26` kg-mol (6260 g-mol if you prefer) original

Iron `699/55.85 = 12.16` kg-mol product

The balanced reaction dictates that the `CO` required is
`3/2 xx 12.16 = 18.24` kg-mol `CO`.

This should be the same for a balanced reaction as
`3 xx 6.26 = 18.78` Kg-mol for complete reaction with the iron oxide.

The moles of `CO_2 = CO` in the equation, so we should have 18.24 kg-mol of `CO_2` product as well (from the stated Fe product amount). From the ideal gas laws we obtain:
V = nRT/P ; `V = (18240 xx 0.0802 xx 273)/1 = 399 xx 10^3L = 399m^3`

You can "mix and match" the other values to decide which ones are "incorrect" OR if you just need to fill the blank with a different number.