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ziro4ka [17]
2 years ago
15

I need help please by answering that question

Chemistry
1 answer:
jenyasd209 [6]2 years ago
5 0
If i can recall it is D
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What is 25 °C in °F?
kifflom [539]

Answer:

77°F

Explanation:

(25°C × 9/5) + 32 = 77°F

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2 years ago
How many sig figs are there<br> 5.00000008
djverab [1.8K]

Answer:

2 sig figs.

Explanation:

Sig Fig Rules:

Any non-zero digit is a significant figure.

Any zeros between 2 non-zero digits are significant figures.

Trailing zeros after the decimal are significant figures.

6 0
3 years ago
based on the general trends on intermolecular forces, rank c2h5oh, hcl, and c3h6 in order of increasing boiling point.
nikklg [1K]
The answer is HCl, C3H6 and C2H5OH. Hydrochloric acid has the lowest boiling point among the three choices since it only has weak dipole-dipole and Van der Waal's forces between molecules which are much weaker than the forces of attraction present in propane and ethanol. Ethanol has the highest since the hydrogen bonding present in ethanol make it hard to break the bonds.
3 0
2 years ago
Read 2 more answers
Why is there a bond between the ions in potassium chloride
yKpoI14uk [10]

Answer:

Explanation:

When the two atoms are in contact, potassium transfers its outer electron to chlorine which readily accepts it, resulting in both atoms achieving a state of eight outermost electrons. With this electron transfer, the ionic bond in KCl is formed.

Hope this helped!!!

6 0
3 years ago
1. A chemist prepares hydrogen fluoride by means of the following reaction:
Natasha_Volkova [10]

Answer:

a) <em>Theoretical Yield of HF = 5.64 grams</em>

b) <em>Percentage Yield = 39%</em>

Explanation:

Reaction Given:

CaF2 + H2SO4 -> CaSO4 + 2HF

CaF2 = 11g

H2SO4 = Used in excess

HF = 2.2 g production = Actual Yield

So, Let's write down the molar masses:

Molar Mass of CaF2 = 78 g /mol

Molar Mass of HF = 20 g/mol

From the reaction, we can see the 1 mole of CaF2 gives the 2 moles of HF

i.e

a) Theoretical Yield of HF:

1 mole CaF2 = 2 moles HF

78 g CaF2 = 2 x 20 g of HF

78 g CaF2 = 40 g of HF

1 g CaF2 = 40g/78g of HF

And in the question it is given that chemist used 11 g of CaF2 so,

1 x 11 g of CaF2 = 11 x 40/78 g of HF

11 g of CaF2 = 440/78 g of HF

11 g of CaF2 = 5.64 g of HF

And this is the theoretical yield

<em>Theoretical Yield of HF = 5.64 grams</em>

b) Now, calculate the Percentage Yield of HF

<em>Percentage Yield = Actual Yield /Theoretical Yield x 100</em>

Percentage Yield = 2.2 g /5.64 g x 100

Percentage Yield = 39%

8 0
2 years ago
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