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Anastasy [175]
3 years ago
12

If a maximum of 5.60g of a gas at 2.50 atm of pressure dissolves in 3.5-L of water, what will the solubility be if the pressure

Chemistry
1 answer:
KonstantinChe [14]3 years ago
6 0
According to Henry's law C = k P
where C = concentration of gas (g/L)
k : Henry's constant
P : pressure of gas above the solution
concentration of gas = 5.6 g / 3.5 L = 1.6 g/L
From Henry's law:
C₁ / C₂ = P₁ / P₂
C₂ = C₁P₂ / P₁ = (1.6 * 5 atm) / 2.5 atm = 3.2 g/L
so the 3.5 L will contain 11.2 g gas

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Compare the charges and masses of protons, neutrons, and electrons.
Eva8 [605]

Answer:

Explanation:

Protons have a positive charge, with a mass of 1 amu.

Neutrons have no charge, also with a mass of 1 amu.

Electrons have a negative charge, with a mass of 1 amu.

This is why when you're calculating the mass of an element or isotope, we only count the number of protons and neutrons.

3 0
3 years ago
10. Hydrogen peroxide (H2O2: M = 34 g mol-1) is a powerful oxidising agent that is used in concentrated solution in rocket fuel
Lubov Fominskaja [6]

Answer:

The molality of solution=12.605 m

Explanation:

We are given that

Molar mass of Hydrogen peroxide, M=34 g/mol

Density of solution, \rho=1.11gcm^{-3}

30% Means mass of solute (Hydrogen peroxide)=30 g

Mass of solvent =100-30=70 g

Total mass of solution, m=100 g

Number of moles of solute=\frac{given\;mass}{molar\;mass}

Using the formula

Number of moles of hydrogen peroxide=\frac{30}{34}

Now, molality of solution

m=\frac{number\;of\;moles\;of\;solute}{mass\;of\;solvent}\times 1000

m=\frac{30}{70\times 34}\times 1000

m=12.605 m

Hence, the molality of solution=12.605 m

6 0
4 years ago
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Bingel [31]

Answer:

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7 0
3 years ago
If the decomposition of a sample of KClO3 produces 3.29 g of O2 , what was the mass (g) of the original sample?
zalisa [80]

Answer: Thus 8.41 g was the mass of the original sample

Explanation:

To calculate the moles :

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

\text{Moles of} O_2=\frac{3.29g}{32g/mol}=0.103moles

2KClO_3\rightarrow 2KCl+3O_2  

According to stoichiometry :

As 3 moles of O_2 are produced by = 2 moles of KClO_3

Thus 0.103 moles of O_2 are produced by =\frac{2}{3}\times 0.103=0.0687moles  of KClO_3

Mass of KClO_3=moles\times {\text {Molar mass}}=0.0687moles\times 122.5g/mol=8.41g

Thus 8.41 g was the mass of the original sample.

3 0
3 years ago
You are attempting to collect pure hydrogen gas by reacting hydrochloric acid with zinc. Based on the amount of reactants you us
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