Which of the following mixture can be separated by sedimentation?

adelina 88 [10]

he balanced equation for the reaction is
4Fe + 3O₂ ---> 2Fe₂O₃
stoichiometry of O₂ to Fe₂O₃ is 3:2

number of O₂ moles used up - mass present / molar mass of O₂
number of O₂ moles = 63.98 g / 32 g/mol = 1.999 mol

if 3 mol of O₂ forms 2 mol of Fe₂O₃
then 1.999 mol of O₂ forms - 2/3 x 1.999 mol = 1.333 mol
answer is A) 1.333 mol of Fe₂O₃ are formed

7 0

4 years ago

Read 2 more answers

Chemists use activity series to determine whether which type of reaction will occur?

bazaltina [42]

Answer:

The correct answer is "single replacement".

Explanation:

The activity series is a representation of a series of metals that are organized according to their order of reactivity. They start from the highest order of reactivity to the lowest order of reactivity.

The purpose of the series is to determine which products are formed in single-displacement reactions. The higher-order metals replace the lower order metals if there are two of them in the same solution. If metal is higher in the series it is more reactive than a metal that is below it in the activity series.

Have a nice day!

5 0

3 years ago

Calculate the amount of heat, in kilojoules, required to turn solid ammonia at -78 degrees Celsius to gaseous ammonia at standar

zhuklara [117]

Answer:

132

Explanation:

3 0

4 years ago

A chemist fills a reaction vessel with 3.82 atm methanol (CH,OH) gas, 7.56 am oxygen (O2) gas, 5.29 atm carbon dioxide (CO2) gas

alisha [4.7K]

Answer: The Gibbs free energy of the given reaction is $1.379\times 10^3kJ$

Explanation:

The equation used to calculate Gibbs free energy change is of a reaction is:

$\Delta G^o_{rxn}=\sum [n\times \Delta G^o_f_{(product)}]-\sum [n\times \Delta G^o_f_{(reactant)}]$

For the given chemical reaction:

$2CH_3OH(g)+3O_2(g)\rightarrow 2CO_2(g)+4H_2O(g)$

The equation for the Gibbs free energy change of the above reaction is:

$\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(CO_2(g))})+(4\times \Delta G^o_f_{(H_2O(g))})]-[(2\times \Delta G^o_f_{(CH_3OH(g))})+(3\times \Delta G^o_f_{(O_2(g))})]$

We are given:

$\Delta G^o_f_{(H_2O(g))}=-228.57kJ/mol\\\Delta G^o_f_{(CO_2(g))}=-394.36kJ/mol\\\Delta G^o_f_{(CH_3OH(g))}=-161.96kJ/mol\\\Delta G^o_f_{(O_2(g))}=0kJ/mol$

Putting values in above equation, we get:

$\Delta G^o_{rxn}=[(2\times (-394.36))+(4\times (-228.57))]-[(2\times (-161.96))+(3\times (0))]\\\\\Delta G^o_{rxn}=-1379.08kJ/mol$

The equation used to Gibbs free energy of the reaction follows:

$\Delta G=\Delta G^o+RT\ln Q_{p}$

where,

$\Delta G$ = free energy of the reaction

$\Delta G^o$ = standard Gibbs free energy = -1379.08 kJ/mol = -1379080 J/mol (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314 J/K mol

T = Temperature = $25^oC=[273+25]K=298K$

$Q_{p}$ = Ratio of concentration of products and reactants = $\frac{(p_{CO_2})^2(p_{H_2O})^4}{(p_{CH_3OH})^2(p_{O_2})^3}$

$p_{CO_2}=5.29atm\\p_{H_2O}=3.89atm\\p_{CH_3OH}=3.82atm\\p_{O_2}=7.56atm$

Putting values in above expression, we get:

$\Delta G=-1379080J/mol+(8.314J/K.mol\times 298K\times \ln (\frac{(5.29)^2\times (3.89)^4}{(3.82)^2\times (7.56)^3}))\\\\\Delta G=-1379039J=1379.039kJ=1.379\times 10^3kJ$

Hence, the Gibbs free energy of the given reaction is $1.379\times 10^3kJ$

5 0

3 years ago

While out on a hike, you find an unknown mineral. How would you test the mineral to find out what it is?

notsponge [240]

Are there answer choices or is it just right it your self?

6 0

4 years ago