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3 years ago

Is a mountain a deconstructive process

Chemistry

1 answer:

blagie [28]3 years ago

6 0

Answer:

yes

Explanation:

i looked it up.........

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Help me with number 19 and 20 please

Doss [256]

19) it's not balanced because when adding h2 and o2 u get h2o2 not h2o
20) I'm not sure

7 0

3 years ago

A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an

inysia [295]

<u>Answer:</u> The molar mass of the unknown compound is 223.2 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

where,

$\pi$ = osmotic pressure of the solution = 8.44 torr

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of solute = ?

R = Gas constant = $62.3637\text{ L torr }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$8.44torr=1\times M\times 62.3637\text{ L. torr }mol^{-1}K^{-1}\times 298K\\\\M=\frac{8.44}{1\times 62.3637\times 298}=4.54\times 10^{-4}M$

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

We are given:

Molarity of solution = $4.54\times 10^{-4}M$

Given mass of unknown compound = 15.2 mg = 0.0152 g (Conversion factor: 1 g = 1000 mg)

Volume of solution = 150.0 mL

Putting values in above equation, we get:

$4.54\times 10^{-4}M=\frac{0.0152\times 1000}{\text{Molar mass of unknown compound}\times 150.0}\\\\\text{Molar mass of unknown compound}=\frac{0.0152\times 1000}{150.0\times 4.54\times 10^{-4}}=223.2g/mol$

Hence, the molar mass of the unknown compound is 223.2 g/mol

5 0

3 years ago

Match the following equation with the type of chemical reaction. Question 6 options: H2 + O2 ---> H2O HBr ---> H2 + Br2 HC

kenny6666 [7]

Hello there!

1. Synthesis: 2H₂ + O₂ → 2H₂O
2. Decomposition: 2HBr → H₂ + Br₂
3. Single-Replacement: 2Al + 3H₂SO₄ → 3H₂ + Al₂(SO₄)₃
4. Double-Replacement: 2HCl + 2NaOH → 2H₂O + 2NaCl
5. Combustion: 2C₂H₆ + 7O₂ → 6H₂O + 4CO₂

I hope this helps!
Brady

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3 years ago

Write the letter of the correct answer on the line

mafiozo [28]

Answer:

D. Vent is the answer please

6 0

2 years ago

Read 2 more answers

Please help me I'm really confused on how to do this. Can someone break it down for me? (stoichiometry)

bazaltina [42]

Answer:

so with every stoichiometry problem with a mass it will make it so you can do the conversion factor with reactants or products.

if you dont understand unit conversions try to study how to set it up. anyways

a.) C12H22O11 has a mass of 342.01 Grams per mole

divide 1.202 G by 342.01 G to get 0.004 miles

b.) you're just taking the AMU of each element in the chemical multiply it by how many there is of it in the chemical, then divide it by the mass of a mole of the chemical.

c.) you take your answers of part b and multiply them by Avogadro's number

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3 years ago