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2 years ago

Can anyone fill in the answers?

Chemistry

1 answer:

Arte-miy333 [17]2 years ago

6 0

Hi, P.S. The atomic number will always be the same as the number of protons...

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Which statement correctly contrasts science and pseudoscience

mojhsa [17]

brainly.com/question/1470976 Hope this helps!

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3 years ago

Do you guys know any cool app for revision apart from quiz let

hammer [34]

Kahoot, there are some pretty great reviews on there but you may need to do some searching

7 0

2 years ago

Ptrpared a solution of sodium chloride (NaCl) by measuring out 49.Umol of sodium chloride into 150. ML. Volumetric flask and fil

ArbitrLikvidat [17]

Answer:

The answer to your question is below

Explanation:

Data

Substance = NaCl

moles of NaCl = 49

volume = 150 ml

Process

Molarity is a unit of concentration that makes a relation of the moles of a substance and the volume.

Molarity = moles / volume (L)

1.- Convert 150 ml to L

1000 ml ------------------ 1 L

150 ml ----------------- x

x = (150 x 1) / 1000

x = 0.15 L

2.- Substitution

Molarity = 49 / 0.15

Molarity = 326. 7

I have a doubt if the number of moles is 49 moles or 49μmoles

4 0

3 years ago

How many atoms are in 578g Na

borishaifa [10]

1.51 x 10²⁵atoms

Explanation:

Given parameters:

Mass of Na = 578g

Unknown:

Number of atoms = ?

Solution:

To find the number of atoms, we must first find the number of moles the given mass contains.

Number of moles = $\frac{mass}{molar mass}$

molar mass of Na = 23g

Number of moles = $\frac{578}{23}$ = 25.13moles

1 mole of a substance = 6.02 x 10²³atoms

25.13 mole of Na = 25.13 x 6.02 x 10²³atoms

This gives 1.51 x 10²⁵atoms of Na

Learn more:

Avogadro's constant brainly.com/question/2746374

#learnwithBrainly

5 0

3 years ago

A meteorologist filled a weather balloon with 3.00L of the inert noble gas helium. The balloon's pressure was 765 torr. The ball

yanalaym [24]

Answer:

4.33 L

Explanation:

Step 1: Given data

Initial volume of the balloon (V₁): 3.00 L

Initial pressure of the balloon (P₁): 765 torr

Final volume of the balloon (V₂): ?

Final pressure of the balloon (P₂): 530 torr

Step 2: Calculate the final volume of the balloon

If we consider Helium to behave as an ideal gas, we can calculate the final volume of the balloon using Boyle's law.

$P_1 \times V_1 = P_2 \times V_2\\V_2 = \frac{P_1 \times V_1}{P_2} = \frac{765torr \times 3.00L}{530torr} = 4.33 L$

7 0

3 years ago