1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
storchak [24]
2 years ago
9

PLEASE HELP ASAP!

Chemistry
1 answer:
egoroff_w [7]2 years ago
3 0

Answer:

Lithium fluoride i think but I am not really sure

But it should be Lithium fluoride

Explanation: that's because neighter boron nor nitrogen contains water

You might be interested in
PRACTICE PROBLEMS
Likurg_2 [28]
72.6g
The density formula is density equal mass divided by volume (d=m/v) to solve this you must get the mass by itself. You do this by multiply volume on both sides which then gets you density times volume equal mass. Then you can plug in the numbers which is 1.20g/mL x 60.5 mL the mL cancels out which leaves you with grams and thus you have 72.6g.
6 0
3 years ago
Given that 25.0 mL of mercury has a mass of 340.0 g, calculate (a) the density of mercury and (b) the mass of 120.0 mL of mercur
natita [175]

Answer :

(a) The density of mercury is, 13.6 g/ml

(b) The mass of 120.0 ml of mercury is, 1632 grams

Explanation :

(a) Now we have to calculate the density of mercury.

<u>Given :</u>

Volume of mercury = 25.0 ml

Mass of mercury = 340.0 g

Formula used :

\text{Density of mercury}=\frac{\text{Mass of mercury}}{\text{Volume of mercury}}

\text{Density of mercury}=\frac{340.0g}{25.0ml}=13.6g/ml

Therefore, the density of mercury is, 13.6 g/ml

(b) Now we have to calculate the mass of 120.0 ml of mercury.

As, 25.0 ml of mercury has mass = 340.0 g

So, 120.0 ml of mercury has mass = \frac{120.0ml}{25.0ml}\times 340.0g=1632g

Therefore, the mass of 120.0 ml of mercury is, 1632 grams

3 0
3 years ago
What is the percent composition by mass of nitrogen in NH4OH?
Juliette [100K]
 <span>the atomic mass of nitrogen is 14. There is 1 nitrogen atom in the molecule so the percentage of N is :

14/35 x100% = 40%</span>
8 0
3 years ago
A chemist has 3.55x1022 molecules of nitrogen monoxide. How
Alina [70]

Answer:

<h2>0.059 moles</h2>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

n =  \frac{N}{L} \\

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

n =  \frac{3.55 \times  {10}^{22} }{6.02 \times  {10}^{23} }  \\  = 0.05897...

We have the final answer as

<h3>0.059 moles</h3>

Hope this helps you

6 0
3 years ago
What would happen to the moon’s interia were to increase? A the moon will fly into space. B the moon will smash into Earth. C th
Montano1993 [528]

Answer:

B

Explanation:

5 0
3 years ago
Other questions:
  • Solid potassium chlorate (kclo3) decomposes into potassium chloride and oxygen gas when heated. how many moles of oxygen form wh
    8·1 answer
  • A compound is known to have an empirical formula of CH and a molecular mass of 78.11 g/ mom what is he molecular formula
    15·1 answer
  • Does the energy go from the surrounding to the chemicals or from the chemicals to the surround in an exothermic reaction?
    6·1 answer
  • Which of the following scenarios is representative of parasitism?
    7·2 answers
  • QUICK CHEMISTRY QUESTION WORTH 15 POINTS WILL MARK BRAINLIEST!
    13·1 answer
  • Please Help Me! Question is on link down below!
    7·1 answer
  • Another student measured the volume of an unmarked water container, obtaining a 35.0% (6pts) Given the actual volume of the cont
    7·1 answer
  • You have a hard glass flask that you plug up with a stopper at room temperature (25 C) and an internal pressure of 1 atm. If you
    8·1 answer
  • How does temperature differ from heat?
    13·1 answer
  • Divers who go to great depths in the ocean experience large differences in pressure between the surface and their final destinat
    6·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!