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3 years ago

What is Density?:

Chemistry

1 answer:

Kryger [21]3 years ago

3 0

Answer:

Density is defined as how tightly or loosely packed a substance is, or to the number of things or people in a certain area.

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By using the titration technique, what can be determined about a given substance?

gtnhenbr [62]

It is strong. it is really strong

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3 years ago

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GIVING 25 POINTS PLUS BRAINLIEST FOR CORRECT ANSWERS!!!!

Airida [17]

Answer:

The answer to your question is:

Explanation:

e) 9.10 x 10³ + 2.2 x 10⁶ = 2.2091 x 10⁶

f) 1113.0 - 14.6 x 10² = -347 = -3.47 x 10²

g) 6.18 x 10⁻⁴⁵ + 4.72 x 10⁻⁴⁴ = 5.338 x 10⁻⁴⁴

h) 4.25 x 10⁻³ - 1.6 x 10⁻² = -0.01175 = -1.175 x 10 ⁻²

5.- Calculate ...

a) 2.63 x 10⁻⁴

b) 2.26 x 10¹³

c) 1.97 x 10²

d) 1.65 x 10⁻²³

e) 2.5 x 10⁻⁸³

f) 1.61 x 10¹⁴

g) 2 x 10⁷⁹

h) 2.37 x 10⁻⁷

7 0

3 years ago

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A compound has a molar mass of 90 grams per mole and the empirical formula CH2O. What is the molecular formula of this compound?

Ira Lisetskai [31]

CH2O = 12 + 2 + 16 = 30
90 /30 = 3
3 x (CH2O) = C3H6O3

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3 years ago

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The solubility of a certain compound in ice-cold water is 0.16 g in 100 mL. Its solubility in hot water is 4.35 g in 100 mL. Wha

jonny [76]

Answer:

96.32 %

Explanation:

Given that:

The solubility of compound in hot water = 4.35 g / 100 mL

The solubility of compound in cold water = 0.16 g / 100 mL

Which means that in 100 mL of hot water, the dissolved compound is 4.35 g and in cold water, the dissolved compound is 0.16 g

Hence, on transition, compound that will catalyze is 4.35 - 0.16 g = 4.19 g

So,

$\%=\frac {4.19}{4.35}\times 100$

Percent recovery for re-crystallization of this compound from water= 96.32 %

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3 years ago

Carlos is making phosphorus trichloride using the equation below. He uses 15.5 g of phosphorus and collects 50.9 g of phosphorus

alex41 [277]

Answer: 35.4 g

Explanation:

The balanced reaction is :

$2P+3Cl_2\rightarrow 2PCl_3$

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of phosphorous}=\frac{15.5g}{31g/mol}=0.50moles$

$\text{Moles of phosphorous chloride}=\frac{50.9g}{137g/mol}=0.372moles$

$2P+3Cl_2\rightarrow 2PCl_3$

According to stoichiometry :

2 moles of phosphorous chloride are produced by = 3 moles of $Cl_2$

Thus 0.37 moles of phosphorous chloride are produced by= $\frac{3}{2}\times 0.372=0.558moles$ of $Cl_2$

Mass of $Cl_2=moles\times {\text {Molar mass}}=0.558moles\times 71g/mol=35.4g$

Thus 35.4 g of chlorine reacted with the phosphorus

5 0

3 years ago

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