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3 years ago

12

It is difficult to measure the correct atomic radius. Why?

1 answer:

Paul [167]3 years ago

4 0

Answer:

its kinda you just need to simplify

Explanation:

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Which pair of atoms has the highest electronegativity difference?

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The best way to accurately determine the pair with the highest electronegativity difference is by using their corresponding electronegativity values. For the each of the choices, the difference is:

A. H-S = 2.5 - 2.1 = 0.4
B. H-Cl = 3 - 2.1 = 0.9
C. N-H = 3 - 2.1 = 0.9
D. O-H = 3.5 - 2.1 = 1.4
E. C-H = 2.5 - 2.1 = 0.4

As show, D. has the highest difference. Without looking at their values, you can also determine the pair with the highest difference by taking note of the trend of electronegativity on the periodic table. Electronegativity increases as you go right a group and up a period. This makes oxygen the most electronegative element among the other elements paired with hydrogen.

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3 years ago

At 400 K, This Reaction Has Kp 8.2 X 104 What Is Kp At 400 K For The Following Reaction

kondor19780726 [428]

The given question is incomplete, here is a complete question.

At 400 K, this Reaction has $K_p=8.2\times 10^{-4}$

$SO_3(g)\rightleftharpoons SO_2(g)+\frac{1}{2}O_2(g)$

What Is $K_p$ at 400 K for the following reaction?

$2SO_3(g)\rightleftharpoons 2SO_2(g)+O_2(g)$

(A) 8.2 x 10⁻⁴

(B) 2.9 x 10⁻²

(C) 6.7 x 10⁻⁷

(D) 1.6 x 10⁻⁷

Answer : The correct option is, (C) $6.7\times 10^{-7}$

Explanation :

The given chemical equation follows:

$SO_3(g)\rightleftharpoons SO_2(g)+\frac{1}{2}O_2(g)$

The equilibrium constant for the above equation, $K_p=8.2\times 10^{-4}$ .

We need to calculate the equilibrium constant for the following equation of above chemical equation, which is:

$2SO_3(g)\rightleftharpoons 2SO_2(g)+O_2(g)$ , $K_p'$

The equilibrium constant for the doubled reaction will be the square of the initial reaction.

Or, we can say that

If the equation is multiplied by a factor of '2', the equilibrium constant will be the square of the equilibrium constant of initial reaction.

The value of equilibrium constant for the following reaction is:

$K_{p}'=(K_p)^2$

$K_{p}'=(8.2\times 10^{-4})^2$

$K_{p}'=6.7\times 10^{-7}$

Hence, the value of equilibrium constant for the following reaction is, $6.7\times 10^{-7}$

7 0

3 years ago