The statements which best describe beta decay are: option 1, 2 and 4.
<h3>What is a beta particle?</h3>
A beta particle can be defined as an isotope which typically undergoes radioactive decay through the emission of a radiation with a -1 charge.
Based on scientific information and records from radioactivity, we can infer that the statements which best describe beta decay are:
- During beta decay, an atom of proton becomes a neutron and a positron.
- During beta decay, an atom of neutron becomes a proton and an electron.
- Beta decay releases energy.
Read more on beta decay here: brainly.com/question/12448836
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54 mL Ba(OH)2x(0.101 mol Ba(OH)2/1000 mL) x (2 mol OH-/ 1 mol Ba(OH)2 ) = 0.0109 mol OH-
0.0109 mol OH-x (1mol HCl/ 1 mol OH- ) = 0.0109 mol HCl
0.109 mol HCl/(0.130 mol/L HCl) = 0.0839 L HCl
0.0839 L HCl * 1000mL = 83.9 mL of 0.130 M HCl
N2 + 3H2 = 2NH3
in this question, we are dealing with only NH3 and H2 so we only focus on that
since the ratio of H2 to 2NH3 is 3:2, we say that
3 liters of H2 = 2 liters of 2NH3
3.6 litres of H2 = x liters of 2NH3
We cross multiple to give:
3 × x = 3.6 × 2
3x = 7.2
Divide both sides by 3
x = 7.2 ÷ 3
x = 2.4liters
Answer:
0.1M NH3
Explanation:
The boiling point of aqueous solutions depend on the nature of intermolecular interactions present. KBr will yield an ionic solution but NH3 will yield a molecular solution having hydrogen bonds. The degree of hydrogen bonding in the aqueous solution will further increase with the concentration of the solution.
Remember that experimental data shows that hydrogen bonds are strong bonds that lead to a significant increase in the boiling point of solutions. Hence 0.1M NH3 solution will have a higher boiling point due to intermolecular hydrogen bonding in the solution.
Answer:
The mass percent of aluminum sulfate in the sample is 16.18%.
Explanation:
Mass of the sample = 1.45 g
Mass of the precipitate = 0.107 g
Moles of aluminum hydroxide = 
According to reaction, 2 moles of aluminum hydroxide is obtained from 1 mole of aluminum sulfate .
Then 0.001372 moles of aluminum hydroxide will be obtained from:
Mass of 0.000686 moles of aluminum sulfate :
= 0.000686 mol × 342 g/mol = 0.2346 g
The mass percent of aluminum sulfate in the sample:
