All categories

3 years ago

For the reaction 2Fe + O2 = 2FeO, how many grams of iron oxide are produced from 8.00 mol of iron? when o2 is an excess

Chemistry

1 answer:

Yanka [14]3 years ago

6 0

Answer:

The answer to your question is 576 grams of FeO

Explanation:

Balanced chemical reaction

2Fe + O₂ ⇒ 2 FeO

Reactant Elements Products

2 Fe 2

2 O 2

Data

mass of FeO = ?

moles of Fe = 8

Excess Oxygen

Process

1.- Convert moles of Fe to grams

Atomic mass = 56 g

56 g of Fe ------------------ 1 mol

x ------------------ 8 moles

x = (8 x 56) / 1

x = 448 g of Fe

2.- Use the coefficients of the balanced reaction to find the grams of FeO.

Molecular mass of FeO = 2[ 56 + 16]

= 144 g

2(56) g of Fe ----------------------- 144 g of FeO

448 g ----------------------- x

x = (448 x 144) / 2(56)

x = 64512 / 112

x = 576 grams of FeO

You might be interested in

The empirical formula of a compound is CH. At 200 degree C, 0.145 g of this compound occupies 97.2 mL at a pressure of 0.74 atm.

Vladimir [108]

Answer:

The molecular formula = $C_{6}H_{6}$

Explanation:

Given that:

Mass of compound, m = 0.145 g

Temperature = 200 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T = (200 + 273.15) K = 473.15 K

V = 97.2 mL = 0.0972 L

Pressure = 0.74 atm

Considering,

$n=\frac{m}{M}$

Using ideal gas equation as:

$PV=\frac{m}{M}RT$

where,

P is the pressure

V is the volume

m is the mass of the gas

M is the molar mass of the gas

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the values in the above equation as:-

$0.74\times 0.0972=\frac{0.145}{M}\times 0.0821\times 473.15$

$M=78.31\ g/mol$

The empirical formula is = $CH$

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 12 + 1 = 13 g/mol

Molar mass = 78.31 g/mol

So,

Molecular mass = n × Empirical mass

78.31 = n × 13

⇒ n ≅ 6

The molecular formula = $C_{6}H_{6}$

6 0

3 years ago

EX/Cupper(I)Iodide

matrenka [14]

Explanation:

Copper sulphate reacts with potassium iodide to form cuprous iodide and iodine.

2CuSO

+4KI→Cu

↓+I

+2K

Thus, CuI

is not formed in this reaction.

Hence, the option B is incorrect and option A is correct.

The liberated iodine is titrated with sodium thiosulphate to form sodium tetrathionate.

2Na

→Na

+2NaI

Iodine is reduced and sodium thiosulphate is oxidized.

4 0

3 years ago

How would adding the catalyst nitrogen monoxide (NO) affect this reaction?

AlladinOne [14]

Answer:

Explanation:

5 0

3 years ago

Read 2 more answers

a steel cylinder is left out in the sun the pressure at 2:00 pm was 1014 kpa at 33.0 c at 7:00 am at a temperature of 21.4c what

e-lub [12.9K]

The easiest way is to use the Law of Gay-Lussac. This law states that there is a direct relation between the temperature in Kelvin of a gas and the pressure.

Then, namig p the pressure and T the temperature in Kelvin and using subscripts for every state:

p/T is constant ==> p_1 / T_1 = p_2/T_2

From which you obtain:

p_2 = [p_1 / T_1] * T_2

T_1 = 33.0 + 273.15 = 306.15 K
T _2 = 21.4 + 273.15 = 294.55 K

p_1 = 1014 kPa

p_2 = 1014 kPa * 294.55 K / 306.15 K = 975.6 kPa

5 0

3 years ago

What contains huge, floating rafts of algae. A. inter tidal area B.coral reef C.estuary

sertanlavr [38]

Best guess would be F or G.

3 0

3 years ago

Read 2 more answers