An example of a fixed cell is a/an

For the reaction

azamat

Answer:

Mass = 5.56 g

Explanation:

Given data:

Mass of Cl₂ = 4.45 g

Mass of NaCl produced = ?

Solution:

Chemical equation:

2Cl₂ + 4NaOH → 3NaCl + NaClO₂ + 2H₂O

Number of moles of Cl₂:

Number of moles = mass/molar mass

Number of moles = 4.45 g/ 71 g/mol

Number of moles = 0.063 mol

Now we will compare the moles of Cl₂ with NaCl.

Cl₂ : NaCl

2 : 3

0.063 : 3/2×0.063 =0.095 mol

Mass of NaCl:

Mass = number of moles × molar mass

Mass = 0.095 mol × 58.5 g/mol

Mass = 5.56 g

7 0

3 years ago

Use of airhole in bunsen burner?

Oksi-84 [34.3K]

Answer:

Image result for Use of airhole in bunsen burner?www.cyberphysics.co.uk

A Bunsen burner, named after Robert Bunsen, is a common piece of laboratory equipment that produces a single open gas flame, which is used for heating, sterilization, and combustion.

Explanation:

3 0

4 years ago

The number of moles in 4.5 x 1024 atoms of oxygen is

Zarrin [17]

(4.5 x 10^24)/(6.02 x 10^23) = 7.475 mol O :)

7 0

3 years ago

1.

Leya [2.2K]

Answer:

V₂ = 530.5 mL

Explanation:

Given data:

Initial temperature = 20.0°C

Final temperature = 40.0 °C

Final volume = 585 mL

Initial volume = ?

Solution:

Initial temperature = 20.0°C (20+273 = 293 K)

Final temperature = 40.0 °C (40+273 = 323 K)

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₁ = V₂T₁ /T₂

V₂ = 585 mL × 293 K / 323 K

V₂ = 171405 mL.K / 323 K

V₂ = 530.5 mL

6 0

3 years ago

A powder contains FeSO4 · 7 H2O (molar mass = 278.01 g/mol), among other components. A 3.055 g sample of the powder was dissolve

solong [7]

Answer:

The mass of FeSO4*7H2O is 1.023 grams

Explanation:

Step 1: Data given

Molar mass of FeSO4 * 7H2O = 278.01 g/mol

Mass of Fe2O3 = 0.294 grams

Mass of the sample = 3.055 grams

Step 2: The balanced equation

4 Fe + 3O2 → 2Fe2O3

Step 3: Calculate moles Fe2O3

Moles Fe2O3 = mass Fe2O3 / molar mass Fe2O3

Moles Fe2O3 = 0.294 grams / 159.59 g/mol

Moles Fe2O3 = 0.00184 moles

Step 3: Calculate moles Fe

In 2 moles Fe2O3 we have 4 moles Fe

For 0.00184 moles we'll have 2*0.00184 = 0.00368 moles

Step 4: The balanced equation

Fe + H2SO4 + 7H2O → FeSO4*7H20 + H2

Step 5: Calculate moles FeSO4* 7H2O

For 1 mol Fe we have 1 mol FeSO4*7H2O

For 0.00368 moles Fe we have 0.00368 moles FeSO4*7H2O

Step 6: Calculate the mass of FeSO4*7H2O

Mass FeSO4*7H2O = moles * molar mass

Mass FeSO4*7H2O = 0.00368 moles * 278.01 g/mol

Mass FeSO4*7H2O = 1.023 grams

The mass of FeSO4*7H2O is 1.023 grams

6 0

3 years ago