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3 years ago

13

Examples for reversible change

2 answers:

castortr0y [4]3 years ago

6 0

Answer:

folding of paper

melting of ice

depletion of ozone

oxidation of blood

Explanation:

Rina8888 [55]3 years ago

4 0

Melting of ice
Sublimation

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The following solutions are prepared by dissolving the requisite amount of solute in water to obtain the desired concentrations.

daser333 [38]

Answer:

C₆H₁₂O₆ < NaCl ≈ CH₃OH < MgCl₂

Step-by-step explanation:

The formula for <em>osmotic pressure</em> (Π) is

Π = icRT

If T is constant,

Π = kic

<em>C₆H₁₂O₆: </em>

Π = k × 1 × 1 = k

<em>MgCl₂: </em>

Π = k × 3 × 1 = 3k

<em>CH₃OH: </em>

Π = k × 1 × 2 = 2k

<em>NaCl: </em>

Π = k × 2 × 1 = 2k

The order of osmotic pressures is

C₆H₁₂O₆ < NaCl ≈ CH₃OH < MgCl₂

8 0

3 years ago

Read 2 more answers

An unknown compound contains only C, H, and O. Combustion of 8.50 g of this compound produced 20.0 g CO2 and 5.46 g H2O. What is

Galina-37 [17]

Answer:

The answer to your question is: C₃H₄O

Explanation:

Data

CxHyOz = 8.5 g

CO2 = 20 g

H2O = 5.46 g

Reaction

CxHyOz + O2 ⇒ CO2 + H2O

CO2

MW = 44g

44g CO2 ----------------- 12g of C

20g CO2 ---------------- x

x = (20 x 12) / 44

x = 5.45 g of C

# of moles = n = 5.45 / 12 = 0.454 mol of C

H2O

MW = 18 g

18 g H2O ------------------- 2g of H

5.46 g -------------------- x

x = (5.46 x 2) / 18 = 0.61 g of H

n = 0.61 / 1 = 0.61 moles of H2

Mass of O2

mass CxHyOz = mass CO2 + mass H2 + mass O2

mass O2 = 8.5 - 5.45 - 0.61

mass O2 = 2.44g

n = 2.44 / 16 = 0.153 mol of O2

Now, divide by the lowest number of moles

0.454 mol of C/ 0.153 = 2.97 ≈ 3

0.61 moles of H2/ 0.153 = 3.99 ≈ 4

0.153 mol of O2/ 0.153 = 1

Then, the empirical formula is: C₃H₄O

7 0

3 years ago

Does Florida get any type of rain?

emmasim [6.3K]

Answer: Florida gets mainly hard downpours or light showers. (i live here so you can trust me)

Explanation:

6 0

3 years ago

Mars have more gravity than earth?<br><br> True or false?

tiny-mole [99]

Answer:

false

Explanation:

earth is larger than mars so it has more gravity

7 0

3 years ago

Read 2 more answers

It takes 42.25 ml of 0.0500 M Na2S2O3 solution to completely react with the iodine present in a 150.0 ml iodine solution. How ma

svlad2 [7]

Answer:

There were 0.268 grams I2 present

Explanation:

Step 1: Data given

Volume of Na2SO3 = 42.25 mL = 0.04225 L

Molarity of Na2SO3 = 0.0500 M

Volume of iodine = 150.0 mL

Step 2: The balanced equation

I2 + 2 Na2SO3 → Na2S2O6 + 2 NaI

Step 3: Calculate moles of Na2SO3

Moles Na2SO3 = molarity * volume

Moles Na2SO3 = 0.0500 M * 0.04225 L

Moles Na2SO3 = 0.0021125 moles

Step 4: Calculate moles I2

For 1 mol I2 we need 2 moles Na2SO3

For 0.0021125 moles Na2SO3 we have 0.00105625

Step 5: Calculate mass of I2

Mass I2 = moles * molar mass

Mass I2 = 0.00105625 * 253.8 g/mol

Mass I2 = 0.268 grams

There were 0.268 grams I2 present

3 0

3 years ago

Read 2 more answers