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Volgvan
2 years ago
5

Which material undergoes radioactive decay?

Chemistry
2 answers:
soldi70 [24.7K]2 years ago
4 0

Answer:

all for nothn ginin all

Explanation:

zhenek [66]2 years ago
4 0
All elements that have a half life
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The compound nicl2 is an ionic compound. what are the ions of which it is composed?
densk [106]
Nickel and chlorine
Ni+
Cl-
3 0
3 years ago
Using the periodic table, answer the following question..How many atoms of neon are in 0.378g of neon (a) 6.02 x 10²³ atoms (b)
zmey [24]

Answer:

B 1.87×10^-²

Explanation:

20.1797 g Neon = 1 mol

0.378 g Neon = y

(Cross multiply)

20.1797y= 0.378 x 1

(Make y the subject of the formula)

y = 0.878/ 20.1787

y = 0.0187317

y = 0.0187 approx

y = 1.87 x 10^-²

7 0
3 years ago
Read 2 more answers
What is the most abundant chemical element in the universe?
Len [333]

hydrogen is the most

5 0
3 years ago
A woman is brought into the emergency room experiencing nausea and vomiting. She is also hyperventilating. She says that she ing
Keith_Richards [23]

Answer:

Protonated form: 96.87%

Unprotonated form: 3.13%

Explanation:

To find the percentage of protoned and unprotoned forms of salicylic acid we must use Henderson-Hasselbalch equation:

pH = pKa + log [A⁻] / [HA]

<em>Where pKa of salicylic acid is 3.49; [A⁻] is the unprotonated form and [HA]:</em>

<em />

2.0 = 3.49 + log [A⁻] / [HA]

0.03236 = [A⁻] / [HA] <em>(1)</em>

And as:

[A⁻] + [HA] = 100% <em>(2)</em>

<em></em>

Replacing (2) in (1):

0.03236 = 100 - [HA] / [HA]

0.03236 [HA] = 100 - [HA]

1.03236[HA] = 100

<h3>[HA] = 96.87%</h3>

And [A⁻]:

[A⁻] = 100 - 96.87

<h3>[A⁻] = 3.13%</h3>

<em></em>

3 0
2 years ago
We know that for a given reaction when the temperature increases from 100 k to 200 k the rate constant doubles. What is the acti
Alenkasestr [34]

Answer:

The activation energy of the reaction is 1.152 kJ/mol.

Explanation:

Activation energy is the minimum amount which is absorbed by the reactant molecules to undergo chemical reaction.

Initial temperature of reaction = T_1=100 K

Final temperature of reaction = T_2=200 K

Initial rate of the reaction at 100 k = K_1=k

Final rate of the reaction at 200 k = K_2=2k

Activation energy is calculated from the formula:

\log\frac{K_2}{K_1}=\frac{E_a}{2.303\times R}(\frac{T_2-T_1}{T_1T_2})

R = Universal gas constant = 8.314 J/ K mol

\log\frac{2k}{k}=\frac{E_a}{2.303\times 8.314 J/K mol}(\frac{200 K-100K}{200 K\times 100K})

E_a=1,152.772 J/mol=1.152 kJ/mol

5 0
3 years ago
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