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3 years ago

A]a[B]b [C]c [D]d

Chemistry

1 answer:

grandymaker [24]3 years ago

8 0

Answer:

When the Keq value is large, the number representing [A]a[B]b must be smaller than the number representing [C]c[D]d. This relationship means that the products must be favored and that the mixture at equilibrium is largely products.

Explanation:

For the equilibrium:

aA + bB ⇄ cC + dD,

Keq = ([C]^c x [D]^d)/([A]ᵃ[B]ᵇ),

For large value of Keq, the value of [C]^c x [D]^d) is larger than that of ([A]ᵃ[B]ᵇ).

So, When the Keq value is large, the number representing [A]a[B]b must be smaller than the number representing [C]c[D]d.

For large value of Keq, the products are favored as the concentration of products is larger than that of reactants at equilibrium.

So, This relationship means that the products must be favored and that the mixture at equilibrium is largely products.

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Two liters of oxygen (O2) is collected over water at 20oC. If the total pressure in the container is 95.00 kPa, what is the part

garri49 [273]

Answer:

THE PARTIAL PRESSURE OF OXYGEN GAS IN THE CONTAINER IS 92.67kPa WHICH IS OPTION B.

Explanation:

To calculate the partial pressure of oxygen gas collected over water, we use

Ptotal = Poxygen + P water

It is worthy to note that when oxygen is collected over water, it is mixed with water vapor and the total pressure in the container will be the sum of the pressure exerted by the oxygen gas and that of the water vapor at that given temperature.

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Using the above formula,

Ptotal = Poxygen + P water

Substituting for Poxygen, we have;

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Read 2 more answers

Ammonium phosphate ((NH4)3PO4) is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H3PO4

Alex Ar [27]

Taking into account the reaction stoichiometry, 8.8488 grams of (NH₄)₃PO₄ is produced by the reaction of 5.82g of phosphoric acid.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

H₃PO₄ + 3 NH₃ → (NH₄)₃PO₄

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

H₃PO₄: 1 mole
NH₃: 3 moles
(NH₄)₃PO₄: 1 mole

The molar mass of the compounds is:

H₃PO₄: 98 g/mole
NH₃: 17 g/mole
(NH₄)₃PO₄: 149 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

H₃PO₄: 1 mole ×98 g/mole= 98 grams
NH₃: 3 moles ×17 g/mole= 51 grams
(NH₄)₃PO₄: 1 mole ×149 g/mole= 149 grams

<h3>Mass of ammonium phosphate formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 98 grams of H₃PO₄ form 149 grams of (NH₄)₃PO₄, 5.82 grams of H₃PO₄ form how much mass of (NH₄)₃PO₄?

mass of (NH₄)₃PO₄= $\frac{5.82 grams of H_{3} PO_{4}x149 grams of (NH_{4} )_{3}PO_{4} }{98 grams of H_{3} PO_{4}}$

mass of (NH₄)₃PO₄= 8.8488 grams

Finally, 8.8488 grams of (NH₄)₃PO₄ is produced by the reaction of 5.82g of phosphoric acid.

Learn more about the reaction stoichiometry:

brainly.com/question/24741074

brainly.com/question/24653699

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