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3 years ago

I need an example of a chemical change involving water.Pleaseeee.

1 answer:

7 0

Chemical change occur when two substances are combined and produces a new substance or decomposes into two or more substances which are entirely different from the original two substances.

There are three types of chemical changes. These are 1) Inorganic Changes, 2) Organic Changes, and 3) Biochemical Changes

Here are some examples of chemicsal changes.

If you combine Sodium and Water, chemical changes causes decomposition into Sodium Hydroxide and Hydrogen.

Sodium + Water ==> Sodium Hydroxide and Hydrogen

Na + H2O ====> NaOH and H

Another example of chemical change is:

Carbon Dioxide and Water will decompose into Sugar and Oxygen

Carbon Dioxide + Water ==> Sugar and Oxygen

CO2 + H2O ==> CnH2nOn (where n is between 3 and 7) and O

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Study the graph in Figure 6.32 and answer to these questions. (see attached image)

Dimas [21]

Hey there :)

We can see that the solubility of salt increases with increasing temperature. This happens with most substances.

To find out the maximum mass of copper sulfate that can be dissolved in water at these temperatures, just interpret the graph.

Considering Y-axis as g copper sulfate/100 g water and the X-axis as the temperature in °C:-

1)

a: 0 °C - 14 g of copper sulfate/100 g of water

b: 50 °C - 34 g of copper sulfate/100 g of water

c: 90 °C - 66 g of copper sulfate/100 g of water

2) From the graph, we can infer that temperature affects the solubility of the salt.

Answered by Benjemin360 :)

3 0

2 years ago

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl ( aq ) , as describe

Nataly [62]

Answer:

0.9483 grams of manganese dioxide should be added to excess HCl.

Explanation:

Pressure of the chlorine gas = P = 795 Torr = 1.046 atm (1 atm = 760 Torr)

Volume of the chlorine gas = V = 255 ml = 0.255 L

Temperature of the chlorine gas = T = 25°C= 298.15 K

Moles of chlorine gas = n

Using ideal gas equation:

PV = nRT

$n=\frac{PV}{RT}=\frac{1.046 atm\times 0.255 L}{0.0821 atm l/mol k\times 298.15 K}$

n = 0.01090 mol

$MnO_2 ( s ) + 4 HCl ( aq)\rioghtarrow MnCl_2 ( aq ) + 2 H_2O ( l ) + Cl_2 ( g )$

According to reaction , 1 mole of chlorine gas is obtained from 1 mole of manganese dioxide.

Then 0.01090 moles of chlorine gas will be obtained from:

$\frac{1}{1}\times 0.01090 mol=0.01090 mol$ manganese dioxide

Mass of 0.01090 moles of manganese dioxide:

0.01090 mol × 87 g/mol = 0.9483 g

8 0

3 years ago

If you are given a 1.0 L (1000mL) of an unknown liquid which has the mass of 500 grams it is most likely which of the above subs

pantera1 [17]

Given in the problem is the mass of the liquid (500 grams) and the volume of the liquid (1000 ml = 1000 cm^3).

We can use these two givens to calculate the density of the liquid using the following rule:
density = mass / volume
density = 500 / 1000 = 0.5 grams / cm^3

Comparing the calculated density with the choices we have, we can deduce that the liquid is most likely to be propane with density 0.494 g / cm^3

6 0

3 years ago

Choose the best description of what's wrong with the following electron configuration for an electrically-neutral atom of sulfur

lions [1.4K]

Answer:

Explanation:

7 0

3 years ago

Read 2 more answers

It takes 500 kJ to remove one mole of electrons from the atoms at the surface of a solid metal. How much energy does it take to

prisoha [69]

Answer:

8.31 × 10⁻²² kJ

Explanation:

Step 1: Given data

Energy required to remove one mole of electrons from the atoms at the surface of a solid metal: 500 kJ/mol e⁻

Step 2: Calculate how much energy does it take to remove a single electron from an atom at the surface of this solid metal

We will use Avogadro's number: there are 6.02 × 10²³ electrons in 1 mole of electrons.

500 kJ/mol e⁻ × 1 mol e⁻/6.02 × 10²³ e⁻ = 8.31 × 10⁻²² kJ/e⁻

7 0

3 years ago