I need help with number 4 and 5 someone plz help

A geochemist in the field takes a 46.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X.

inysia [295]

Answer:

The solubility of the mineral compound X in the water sample is 0.0189 g/mL.

Explanation:

Step 1: Given data

The volume of water sample = 46.0 mL.

The weight of the mineral compound X after evaporation, drying, and washing = 0.87 g.

Step 2: Calculate the solubility of X in water

46.00 mL of water sample contains 0.87 g of the mineral compound X.

To calulate how many grams of the mineral compound 1.0 mL of water sample contains:

0.87 g/46.0 mL = 0.0189 g.

This means the solubility of the mineral compound X in the water sample is 0.0189 g/mL.

3 0

3 years ago

Using the Law of Conservation of Matter, determine the number of grams of iron sulfide (FeS) that will be produced in this react

vazorg [7]

The Law of Conservation of Mass states that the mass of reactants entering a reaction must be equal to the mass of the products exiting it. In this case, we only have 2 reactants, Fe and S, and we only have 1 product, FeS. Therefore we expect the total mass of the Fe and S reactants to equal the mass of FeS. This gives us 112 g + 64 g = 176 g of FeS, which is choice D.

4 0

3 years ago

Read 2 more answers

4.41 g of propane gas (C3H8) is injected into a bomb calorimeter and ignited with excess oxygen, according to the reaction below

gayaneshka [121]

Answer : The heat of the reaction is -221.6 kJ

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter

$q_{rxn}=-q_{cal}$

$q_{cal}=c_{cal}\times \Delta T$

where,

$q_{rxn}$ = heat released by the reaction = ?

$q_{cal}$ = heat absorbed by the calorimeter

$c_{cal}$ = specific heat of calorimeter = $97.1kJ/^oC=97100J/^oC$

$\Delta T$ = change in temperature = $(T_{final}-T_{initial})=(27.282-25.000)=2.282^oC$

Now put all the given values in the above formula, we get:

$q_{cal}=(97100J/^oC)\times (2.282^oC)$

$q_{cal}=221582.2J=221.6kJ$

As, $q_{rxn}=-q_{cal}$

So, $q_{rxn}=-221.6kJ$

Thus, the heat of the reaction is -221.6 kJ

6 0

3 years ago

What is the molar mass of Al2(SO4)3

umka21 [38]

Answer:

The molar mass of $Al_2(SO_4)_3$ is 342.145 g/mol

Explanation:

The molar mass is stated as the “mass per unit amount of substance”of a given chemical compound

$Al_2(SO_4)_3$ is Aluminium sulphate. They easily dissolve in water. It is primarily used as a 'coagulating agent' in the drinking water purification and also in waste and sewage water treatment plants,

We know,

Atomic weight of Aluminium = 26.981

Atomic weight of Sulphur= 32.065

Atomic weight of Oxygen = 15.9994

Now molar mass of $Al_2(SO_4)_3$ (Aluminium sulphate) is

=>2(26.981)+3(32.065+4(15.999))

=>53.962 +3(32.065+63.996)

=>53.962+3(96.061)

=>53.962+288.183

=>342.145

4 0

3 years ago

The empirical formula of the sugar glucose is ch2o. if the relative molecular mass of glucose is measured to be 180.16 g/mol the

ZanzabumX [31]

Answer:

18016

Explanation:

(empirical formula)n=molar mass

7 0

2 years ago