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torisob [31]
3 years ago
5

Of the choices below, which is true for the relationship shown? it is ka for the acid h3p2o72â. it is kb for the acid h3p2o72â.

it is ka for the acid h2p2o72â. it is kb for the acid h2p2o72â
Chemistry
2 answers:
VARVARA [1.3K]3 years ago
7 0
It is Ka<span> for the acid H</span>3P2O7<span>2</span>
Semenov [28]3 years ago
3 0
A For PLATO. just did it
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When you apply heat energy to a substance, where does the energy go? Think about the law of conservation of energy.
Softa [21]

Answer:

the heat energy is transformed to any kind of energy depending on what it's meant to be transformed to.

remember it cannot be destroyed so it's definitely transformed to some kinda energy

8 0
3 years ago
g Suppose a 49. L reaction vessel is filled with 1.5 mol of NO. What can you say about the composition of the mixture in the ves
irakobra [83]

The question is incomplete, the complete question is:

At a certain temperature, the equilibrium constant K_{eq} for the following reaction is 0.74:

NO_3(g)+NO(g)\rightleftharpoons 2NO_2(g)

Suppose a 49.0 L reaction vessel is filled with 1.5 mol of NO_3 and 1.5 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium?  

A. There will be very little NO_3 and NO.

B. There will be very little NO_2

C. Neither of the above is true.

<u>Answer:</u> The correct option is B. there will be very little NO_2

<u>Explanation:</u>

We are given:

Initial moles of NO_3 = 1.5 moles

Initial moles of NO = 1.5 moles

Volume of vessel = 49 L

As, moles of reactants and moles of products are equal, the volume term will not appear in the equilibrium constant expression.

Equilibrium constant for the reaction = 0.74

For the given chemical equation:

                                  NO_3(g)+NO(g)\rightleftharpoons 2NO_2(g)

Initial:                            1.5           1.5             -

At eqllm:                     1.5-x        1.5-x            2x

The expression of equilibrium constant for the above reaction:

K_{eq}=\frac{[NO_2]^2}{[NO_3]\times [NO]}

Putting values in above equation, we get:

0.74=\frac{(2x)^2}{(1.5-x)(1.5-x)}\\\\x=-1.13, 0.451

Neglecting the negative value of equilibrium constant because concentration cannot be negative

Equilibrium concentration of NO_3 = (1.5 - x) = (1.5 - 0.451) = 1.049 moles

Equilibrium concentration of NO = (1.5 - x) = (1.5 - 0.451) = 1.049 moles

Equilibrium concentration of NO_2 = 2x = (2\times 0.451)=0.902mol

There are 3 possibilities:

  • If K_{eq}, the reaction is reactant favored
  • If K_{eq}>1, the reaction is product favored.
  • If K_{eq}=1, the reaction is in equilibrium.

Here, the value of K_{eq}=0.74, which is less than 1, therefore the reaction is reactant favored and we can say that there will be very little NO_2.

Hence, the correct option is B. there will be very little NO_2

7 0
2 years ago
Which of the following is the best explanation for a covalent bond?
Scrat [10]

Answer:

A. electrons simultaneously attracted by more than one nucleus

Explanation:

  • Covalent bond is the bond which is formed with the sharing of the electrons between the two atoms which are taking part in the bond. It is generally formed between the atoms with similar electronegativity values.
  • It is the bond which is generally occurs within non metals as they share electrons to complete their octet.
  • The difference in the electronegativity values of the atoms involving in a covalent bond must not exceed the value of 1.7 .

Thus, the electrons are attracted by the two different nucleus of the atoms that are taking part in the bonding.

<u>So, the correct answer is:- A. electrons simultaneously attracted by more than one nucleus</u>

6 0
3 years ago
The enthalpy change for the explosion of ammonium nitrate with fuel oil is –7198 kJ for every 3 moles of NH4NO3. What is the ent
anastassius [24]

Answer:

−2399.33 kJ

Explanation:

If NH₄NO₃ reacts with fuel oil to give a ΔH of -7198 for every 3 moles of NH₄NO₃

What is the enthalpy change for 1.0 mole of NH₄NO₃ in this reaction

∴ For every 1 mole, we will have \frac{1}{3} of the total enthaply of the 3 moles

so, to determine the 1 mole; we have:

\frac{1}{3}*(-7198kJ)

= −2399.33 kJ

∴ the enthalpy change for 1.0 mole of NH₄NO₃ in this reaction = −2399.33 kJ

7 0
3 years ago
What is the atomic mass equal to?
mixer [17]

Atomic mass is equal to the total number of electrons  neutrons and protons

8 0
3 years ago
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