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Nezavi [6.7K]
2 years ago
8

For most substances, the distance between the particles is smallest when the substance

Chemistry
1 answer:
olchik [2.2K]2 years ago
3 0
Is a solid? has strong intermolecular forces? 
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For the following reaction, identify whether the compound in bold is behaving as an acid or a base.
harina [27]

Answer: acid

Explanation: it dissolves in water to produce hydronium ion as the only positive ion

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3 years ago
What is the correct electron configuration for oxygen?
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It would be: 1s2, 2s2, 2p4
3 0
3 years ago
Does the following compound contain a polyatomic ion? Na2SO4<br> Yes<br> No
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The answer is yes I believe so.
8 0
2 years ago
Which type of equilibrium exists in a sealed flask containing Br2(ℓ) and Br2(g) at 298 K and 1.0 atm?(1) static phase equilibriu
marishachu [46]
The correct answer is 3.

A dynamic phase equilibrium is when a reversible reaction no longer changes its ratio of reactants to products. However, substances continue to move between the chemicals at an equal rate, which means the net change is 0. This is known as a steady state.
8 0
3 years ago
2 NO + O22 NO2 is second order in NO and first order in O2. Complete the rate law for this reaction in the box below. Use the fo
riadik2000 [5.3K]

Answer : The value of rate of reaction is 1.35\times 10^{-8}Ms^{-1}

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

The given chemical equation is:

2NO+O_2\rightarrow 2NO_2

Rate law expression for the reaction is:

\text{Rate}=k[NO]^a[O_2]^b

As per question,

a = order with respect to NO  = 2

b = order with respect to O_2 = 1

Thus, the rate law becomes:

\text{Rate}=k[NO]^2[O_2]^1

Now, calculating the value of rate of reaction by using the rate law expression.

Given :

k = rate constant = 9.87\times 10^3M^{-2}s^{-1}

[NO] = concentration of NO = 7.86\times 10^{-3}M

[O_2] = concentration of O_2= 2.21\times 10^{-3}M

Now put all the given values in the above expression, we get:

\text{Rate}=(9.87\times 10^3M^{-2}s^{-1})\times (7.86\times 10^{-3}M)^2\times (2.21\times 10^{-3}M)^1

\text{Rate}=1.35\times 10^{-8}Ms^{-1}

Hence, the value of rate of reaction is 1.35\times 10^{-8}Ms^{-1}

7 0
2 years ago
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