All categories

3 years ago

Which picture best illustrates thermal energy transfer by conduction?

Chemistry

2 answers:

leva [86]3 years ago

8 0

Answer:

hahuduhshhshxgushs hxushhzuwhysgsh

netineya [11]3 years ago

6 0

Metal Spoon in Hot Water

You might be interested in

a cell on a microscope slide and noticed cell walls and cell membrane bound organelles. the students conclude the cells are what

lord [1]

The students conclude the cells are plant cells.

7 0

3 years ago

When you hold a container, where should the label be?

beks73 [17]

Answer:

On the outside or something like that

7 0

3 years ago

Is a blood vessel an organ

Alika [10]

Yes, but they are tubular organs and like all other organs are made up of tissues

7 0

3 years ago

Read 2 more answers

Which one of these samples contains the smallest number of molecule?

erma4kov [3.2K]

Answer:

E) 1.0L of He at STP

Explanation:

8 0

4 years ago

Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of alumin

Lerok [7]

<u>Answer:</u> The percentage yield of HF is 73.36 %

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

For calcium fluoride:

Given mass of calcium fluoride = 6.25 kg = 6250 g (Conversion factor: 1 kg = 1000 g)

Molar mass of calcium fluoride = 78.07 g/mol

Putting values in above equation, we get:

$\text{Moles of calcium fluoride}=\frac{6250g}{78.07g/mol}=80.05mol$

For the given chemical reaction:

$CaF_2+H_2SO_4\rightarrow CaSO_4+2HF$

By Stoichiometry of the reaction:

1 mole of calcium fluoride produces 2 moles of hydrofluoric acid

So, 80.05 moles of calcium fluoride will produce = $\frac{2}{1}\times 80.05=160.1mol$ of hydrofluoric acid

Now, calculating the theoretical yield of hydrofluoric acid using equation 1, we get:

Moles of of hydrofluoric acid = 160.1 moles

Molar mass of hydrofluoric acid = 20.01 g/mol

Putting values in equation 1, we get:

$160.1mol=\frac{\text{Theoretical yield of hydrofluoric acid}}{20.01g/mol}=3203.6g=3.20kg$

To calculate the percentage yield of hydrofluoric acid, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of hydrofluoric acid = 2.35 kg

Theoretical yield of hydrofluoric acid = 3.20 kg

Putting values in above equation, we get:

$\%\text{ yield of hydrofluoric acid}=\frac{2.35g}{3.20g}\times 100\\\\\% \text{yield of hydrofluoric acid}=73.36\%$

Hence, the percentage yield of HF is 73.36 %

4 0

3 years ago