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bogdanovich [222]
3 years ago
10

Select the correct answer.

Chemistry
2 answers:
Black_prince [1.1K]3 years ago
6 0
The answer is C. silicon , hope this helps!
Lelechka [254]3 years ago
5 0

Answer:

hf and si

Explanation:

hope that helped

You might be interested in
What is true if a liquid and a gas are in equilibrium?
MAXImum [283]

Answer:

A - Liquid molecules forming a gas and gas molecules forming a

liquid are equal in number.

Explanation:

A P E X

6 0
3 years ago
What mass of f2 is needed to produce 120. g of pf3 if the reaction has a 78.1% yield?
lesya692 [45]

write the equation for the reaction

that is 6 F2 +P4 =4 PF3

find the theoretical mass that is

let the theoretical yield be represented by y

theoretical yield = 78.1/100 = 120/y

y= 153.6 grams

find the number of moles of  PF3

moles = mass/molar mass

= 153.6/87.97 =1.746 moles

by use of mole ratio between  F2 :PF3 which is 6:4 the moles of F2 is therefore= 1.746 x 6/4 = 2.62 moles

mass = moles x molar mass

= 1.746 moles x38 g/mol = 99.6 grams

6 0
3 years ago
Can I please Get Help with this question ‍♂️ ?
Nitella [24]

Answer:

Mg(NO4)2 is 180.3 g/mol

Explanation:

First find the substance formula.

Magnesium Nitrate.

Magnesium is a +2 charge.

Nitrate is a -1 charge.

So to balance the chemical formula,

We need 1 magnesium atom for every nitrate atom.

2(1) + 1(-2) = 0

So the substance formula is Mg(NO4)2.

Now find the molar mass of Mg(NO4)2.

Mg = 24.3 amu

N = 14.0 amu

O = 16.0 amu

They are three nitrogen and twelve oxygen atoms.

So you do this: 24.3 + 14.0(2) + 16.0(8) = 180.3 g/mol

So the molar is mass is 180.3 g/mol.

The final answer is Mg(NO4)2 is 180.3 g/mol

Hope it helped!

7 0
3 years ago
3 points
VLD [36.1K]

Answer:

<h3>The answer is 8.29 %</h3>

Explanation:

The percentage error of a certain measurement can be found by using the formula

P(\%) =  \frac{error}{actual \:  \: number}  \times 100\% \\

From the question

actual density = 19.30g/L

error = 20.9 - 19.3 = 1.6

We have

p(\%) =  \frac{1.6}{19.3}  \times 100 \\  = 8.290155440...

We have the final answer as

<h3>8.29 %</h3>

Hope this helps you

5 0
3 years ago
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as
zubka84 [21]

Answer:

Explanation:

MnO₂(s) + 4 HCl(aq)  = MnCl₂(aq) + 2 H₂O(l) + Cl₂

87 g                                                                     22.4 x 10³ mL

volume of given chlorine gas at NTP or at 760 Torr and 273 K

=  175 x ( 273 + 25 ) x 715 / (273 x 760 )

= 179.71 mL

22.4 x 10³ mL of chlorine requires 87 g of MnO₂

179.4 mL of chlorine will require    87 x 179.4 / 22.4 x 10³ g

= 696.77 x 10⁻³ g

= 696.77 mg .

6 0
3 years ago
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