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Vikentia [17]
2 years ago
11

What is the empirical formula for a compound if a sample contains 1.0 g of S and 1.5 g of O?

Chemistry
1 answer:
sammy [17]2 years ago
6 0
I think it’s SO3 I’m not quite sure though
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Compare and contrast alpha beta and gamma radiation
Evgen [1.6K]
There are usually 3 topics used to compare types of radiation: 

Ionising ability
Penetrative power 
Range in air

Ionising ability
Alpha radiation has strong ionising ability, while beta only has moderate ionisation and gamma is very weakly ionising.

Penetrative power 
Alpha particles are weakly penetrating, stopped by paper, while beta particles have stronger penetrating ability, stopped by skin and gamma radiation is very strongly penetrating, stopped only by thick layers of lead.

Range in air
Alpha particles- range of only a few centimetres
Beta - range of up to one meter 
Gamma- infinite range in air.

Hope this helps:)


8 0
3 years ago
BaCl2(aq) + Na2CO3(aq) BaCO3(s) + NaCl(aq
Vitek1552 [10]
This is the equation balanced:

<span>BaCl2(aq) + Na2CO3(aq) = BaCO3(s) + 2 NaCl(aq)

Then the coefficient in front of Na Cl is 2.

Answer: 2
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7 0
3 years ago
Which of these compounds are oxidizing agents?
elena55 [62]

i guess its e) Mn (VII)

if it was wrong pls let me knw


6 0
3 years ago
Read 2 more answers
(WILL GIVE BRAINLIEST IF YOU ANSWER ALL 4) Chemistry
Kitty [74]

Answer:

See explanations

Explanation:

a. Molarity = moles/Volume in Liters = 5moles/2Liters = 2.5M in NaCl

b. Freezing Pt Depression

     1. Sprinkling salt on icy surfaces

    2. Using antifreeze in automobile cooling systems

    3. <em>Not an application </em>

    4. Using salt to make ice cream

c. pOH = -log[OHˉ] = -log(1x10ˉ¹⁰) = -(-10) = 10 => pH = 14 – pOH = 14 – 10 = 4

d. H₂O + NH₃ => NH₄⁺ + OHˉ => Bronsted Acid is H₂O  (proton donor)

5 0
3 years ago
Assuming that gasoline is 100% isooctane, that isooctane burns to produce only CO2CO2 and H2OH2O, and that the density of isooct
Aleksandr [31]

Answer:

1.12×10¹¹ kg of CO₂ are produced with 4.6×10¹⁰ L of isooctane

Explanation:

Let's state the combustion reaction:

C₈H₁₈  +  25/2O₂  →   8CO₂  +  9H₂O

Let's calculate the mass of isooctane that reacts.

Density = Mass / Volume

Density . Volume = Mass

First of all, let's convert the volume in L to mL, so we can use density.

4.6×10¹⁰ L . 1000 mL / 1L = 4.6×10¹³ mL

0.792 g/mL . 4.6×10¹³ mL = 3.64 ×10¹³ g

This mass of isooctane reacts to produce CO₂ and water, so let's determine the moles of reaction

3.64 ×10¹³ g . 1mol / 114 g = 3.19×10¹¹ mol

Ratio is 1:8 so 1 mol of isooctane can produce 8 moles of dioxide

Therefore 3.19×10¹¹ mol would produce (3.19×10¹¹ mol . 8)  = 2.55×10¹² moles of CO₂

Now, we can determine the mass of produced CO₂ by multipling:

moles . molar mass

2.55×10¹² mol . 44 g/mol = 1.12×10¹⁴ g of CO₂

If we convert to kg  1.12×10¹⁴ g / 1000 =  1.12×10¹¹ kg

6 0
3 years ago
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