All categories

2 years ago

How many moles of KCIO3 are in 5 g of KClO3?

2 answers:

7 0

1. Calculate the molar mass of KClO3: 39.098+ 35.453 + 3(16) = 122.551 g KClO3
2. 5gKClO3 x 1mol KClO3/ 122.551g KClO3 = 0.041mol of KClO3

STatiana [176]2 years ago

6 0

Molar mass of KClO3

$\\ \tt\hookrightarrow 39+35+3(16)$

$\\ \tt\hookrightarrow 74+48$

$\\ \tt\hookrightarrow 122g/mol$

Now

$\\ \tt\hookrightarrow No\:of\:moles=\dfrac{Given\:mass}{Molar\:mass}$

$\\ \tt\hookrightarrow No\:of\:moles=\dfrac{5}{122}$

$\\ \tt\hookrightarrow No\:of\:moles=0.04mol$

You might be interested in

What is the anion of the compound Cu(CH3COO)2?

olya-2409 [2.1K]

Answer:

The anion of the compound is b CH3COO-

Explanation:

The compound cupric acetate Cu(CH3COO)2 undergo dissociation to form cupric ion Cu2+ and Acetate anion(CH3COO-)

Cu(CH3COO)2⇒ Cu2+ + CH3COO-

From the above equation it can be stated that the anion of Cu(CH3COO)2 is CH3COO-.

4 0

2 years ago

Predict which of the substances, NH3, N2, CH2Cl2, Cl2, CCl4 has

gulaghasi [49]

Answer:

djsjwjwjdjxjdbs djwuqidx8diw d xbd

6 0

3 years ago

A gas exerts a pressure of 1.8 atm at a temperature of 60 degrees celsius. What is the new temperature when the pressure of the

Kamila [148]

The answer for the following problem is mentioned below.

Therefore the final temperature of the gas is 740 K

Explanation:

Given:

Initial pressure of the gas ( $P_{1}$ ) = 1.8 atm

Final pressure of the gas ( $P_{2}$ ) = 4 atm

Initial temperature of the gas ( $T_{1}$ ) = 60°C = 60 + 273 = 333 K

To solve:

Final temperature of the gas ( $T_{2}$ )

We know;

From the ideal gas equation;

we know;

P × V = n × R × T

So;

we can tell from the above equation;

P ∝ T

(i.e.)

$\frac{P}{T}$ = constant

$\frac{P_{1} }{P_{2} }$ = $\frac{T_{1} }{T_{2} }$

Where;

$P_{1}$ = initial pressure of a gas

$P_{2}$ = final pressure of a gas

$T_{1}$ = initial temperature of a gas

$T_{2}$ = final temperature of a gas

$\frac{1.8}{4}$ = $\frac{333}{T_{2} }$

$T_{2}$ = $\frac{333*4}{1.8}$

$T_{2}$ = 740 K

Therefore the final temperature of the gas is 740 K

8 0

3 years ago

A student dissolves of glucose in of a solvent with a density of . The student notices that the volume of the solvent does not c

nikitadnepr [17]

Answer:

0.052 M

0.059 m

Explanation:

There is some missing info. I think this is the complete question.

A student dissolves 4.6 g of glucose in 500 mL of a solvent with a density of 0.87 g/mL. The student notices that the volume of the solvent does not change when the glucose dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits.

Step 1: Calculate the moles of glucose (solute)

The molar mass of glucose is 180.16 g/mol.

4.6 g × 1 mol/180.16 g = 0.026 mol

Step 2: Calculate the molarity of the solution

0.026 moles of glucose are dissolved in 500 mL (0.500 L) of solution. We will use the definition of molarity.

M = moles of solute / liters of solution

M = 0.026 mol / 0.500 L = 0.052 M

Step 3: Calculate the mass corresponding to 500 mL of the solvent

The solvent has a density of 0.87 g/mL.

500 mL × 0.87 g/mL = 435 g = 0.44 kg

Step 4: Calculate the molality of the solution

We will use the definition of molality.

m = moles of solute / kilograms of solvent

m = 0.026 mol / 0.44 kg = 0.059 m

4 0

3 years ago

Which statement best explains why the elements in Group 18 do not have electronegativity values?

Gnesinka [82]

Answer:

1) The elements have filled valence levels.

Explanation:

Since they have filled valence levels, they're stable and don't need to electrons to fill their valence shells since they're already full.

2) False, They do have electrons

3) False, He does have only one electron shell, but going down the periods, every next element have one more electron shell than a preceding one has.

4)False, they're actually the smallest atoms of their respective period

5 0

2 years ago