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3 years ago

What happens to a ionic compound when it has fully been dissolved in water?

1 answer:

3 0

We'll look at what happens when you dissolve ionic and covalent compounds in water. Ionic compounds break apart into the ions that make them up, a process called dissociation, while covalent compounds only break into the molecules, not the individual atoms.When you immerse an ionic compound in water, the ions are attracted to the water molecules, each of which carries a polar charge. If the attraction between the ions and the water molecules is great enough to break the bonds holding the ions together, the compound dissolves

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Lisa needs to buy a helium tank to fill up all the balloons. If the helium must be compressed from an original volume of 27.0L a

algol13

Answer:

$P_2=135.73psi$

Explanation:

Hello,

In this case we use the Boyle's law which allows us to understand the volume-pressure behavior as an inversely proportional relationship:

$V_1P_1=V_2P_2$

Whereas we solve for $P_2$ as the required final pressure:

$P_2=\frac{V_1P_1}{V_2} =\frac{27.0L*14.7psi}{3.00L}\\ \\P_2=135.73psi$

Best regards.

7 0

3 years ago

Read 2 more answers

Which element is most reactive sodium,magnesium, or aluminum and why?

ludmilkaskok [199]

Magnesium would be more reactive.

6 0

3 years ago

112 g of aluminum carbide react with 174 g water to produce methane and aluminum hydroxide in the reaction shown below.

dolphi86 [110]

Answer: 4.999 moles of excess reactant will be left over.

Explanation:

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of aluminium carbide = 112 g

Molar mass of aluminium carbide = 143.96 g/mol

Putting values in equation 1:

$\text{Moles of aluminium carbide}=\frac{112g}{143.96g/mol}=0.778mol$

For the given chemical reaction:

$2Al_4C_3(s)+12H_2O(l)\rightarrow 3CH_4(g)+4Al(OH)_3(s)$

By the stoichiometry of the reaction:

2 moles of aluminium carbide reacts with 12 moles of water

So, 0.778 moles of aluminium carbide will react with = $\frac{12}{2}\times 0.778=4.668 mol$ of water

Given mass of water = 174 g

Molar mass of water = 18 g/mol

Putting values in equation 1:

$\text{Moles of water}=\frac{174g}{18g/mol}=9.667mol$

Moles of excess reactant (water) left = 9.667 - 4.668 = 4.999 moles

Hence, 4.999 moles of excess reactant will be left over.

8 0

2 years ago

How many liters of 4M solution can be made using 100 grams of lithium bromide

uysha [10]

Molar mass of LiBr (mm )= 86.845 g/mol

Molarity ( M ) = 4 M

Mass of solute ( m ) = 100 g

Volume ( V ) = in liters ?

V = m / mm * M

V = 100 / 86.845 * 4

V = 100 / 347.38

V = 0.2875 L

hope this helps!.

5 0

3 years ago

ASAP I AM GIVING BRAINLIEST PLEASEEEEEEEEE HELPPPPPPPPPPPPPPPPPP

zepelin [54]

Answer:

Explanation:

In the example, the amount of hydrogen is 202,650 x 0.025 / 293.15 x 8.314472 = 2.078 moles. Use the mass of the hydrogen gas to calculate the gas moles directly; divide the hydrogen weight by its molar mass of 2 g/mole. For example, 250 grams (g) of the hydrogen gas corresponds to 250 g / 2 g/mole = 125 moles.

7 0

3 years ago