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3 years ago

Determine the volume occupied by 2.5 mol of a gas at 18 °C if the pressure is 81.8 kPa?

Chemistry

1 answer:

mars1129 [50]3 years ago

3 0

Answer:

74 litre

Explanation:

using ideal gas eqation PV=nRT

here P(pressure)=81.8 kPa =81.8×10^3 Pa

moles=2.5

temperature=273.15+18=291.15K

Gas constant R=8.314m^3-Pa/K-mol

now, V=nRT/P = 8.314×2.5×291.5/81.8×10^3 ≈74litre

✌️;)

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In the equation CH4 + 2O2 --> 2H2O + CO2 What is the mass of CO2 produced when 35g of O2 reacts?

Anestetic [448]

Answer:

24.06 g of CO₂

Explanation:

The balanced equation for the reaction is given below:

CH₄ + 2O₂ —> 2H₂O + CO₂

Next, we shall determine the mass of O₂ that reacted and the mass of CO₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of O₂ = 2 × 16 = 32 g/mol

Mass of O₂ from the balanced equation = 2 × 32 = 64 g

Molar mass of CO₂ = 12 + (2×16)

= 12 + 32

= 44 g/mol

Mass of CO₂ from the balanced equation = 1 × 44 = 44 g

SUMMARY:

From the balanced equation above,

64 g of O₂ reacted to produce 44 g of CO₂.

Finally, we shall determine the mass of CO₂ produced by the reaction of 35 g of O₂. This can be obtained as follow:

From the balanced equation above,

64 g of O₂ reacted to produce 44 g of CO₂.

Therefore, 35 g of O₂ will react to produce = (35 × 44)/64 = 24.06 g of CO₂.

Thus, 24.06 g of CO₂ were produced from the reaction.

8 0

2 years ago

I don’t get it How do you solve the problems

pogonyaev

It would be D, 90.0 g

5 0

3 years ago

The lattice energy of a salt is related to the energy required to separate the ions. For which of the following pairs of ions is

Kay [80]

Answer: The Lattice energy is the energy required to separate an ionic solid into its component gaseous ions or

It is the energy released when gaseous ions combine to form an ionic solid.

Explanation:

The lattice energy depends on the ionization energies and electron affinities of atoms involved in the formation of the compound. The ionization energies and electron affinities also depends on the ionic radius and charges of the ions involved. As the ionic radius for cations increases down the groups, ionization energy decreases, whereas, as ionic radii decreases across the periods , ionization energy increases. The trend observed for anions is that as ionic radii increase down the groups, electron affinity decreases. Across the period, as ionic radii increases electron affinity increases. Also, as the charge on the ion increases, it leads to an increase in energy requirement/content.

Therefore, for compounds formed from cations and anions in the same period, the highest charged cation and anion will have the highest lattice energy. For example, among the following compounds: Al2O3 (aluminium oxide), AlCl3 (aluminium chloride), MgO, MgCl2 (magnesium chloride), NaCl, Na2O (sodium oxide); Al2O3(aluminium oxide) will have the highest lattice energy, thus will be hardest to break apart because its ions have the highest charge.

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2 years ago

In the process of eukaryotic pre-mRNA splicing, how is the lariat intermediate formed?

Aleks [24]

Answer:

Explanation:

The Eukaryotic pre-mRNA receives a 5' cap and 3'poly(A) tail before Introns are removed and the mRNA is considered ready for translation.

4 0

2 years ago

As you have seen, ozone is formed in the upper atmosphere through the reaction:

baherus [9]

The rate law equation for Ozone reaction

r=k[O][O₂]

<h3>Further explanation</h3>

Given

Reaction of Ozone :.

O(g) + O2(g) → O3(g)

Required

the rate law equation

Solution

The rate law is a chemical equation that shows the relationship between reaction rate and the concentration / pressure of the reactants

For reaction

aA + bB ⇒ C + D

The rate law can be formulated:

$\large{\boxed{\boxed{\bold{r~=~k.[A]^a[B]^b}}}$

where

r = reaction rate, M / s

k = constant, mol¹⁻⁽ᵃ⁺ᵇ⁾. L⁽ᵃ⁺ᵇ⁾⁻¹. S⁻¹

a = reaction order to A

b = reaction order to B

[A] = [B] = concentration of substances

So for Ozone reaction, the rate law (first orde for both O and O₂) :

$\tt \boxed{\bold{r=k[O][O_2]}}$

5 0

3 years ago