<span>The statement is false. It was Democritus, a Greek
philosopher, who first theorized that matter was ultimately composed of atoms.
His ideas were not widely accepted in his time (460-370 B.C), but during the 19th
century, John Dalton proposed this theory and gained broad acceptance.</span>
Answer:
Passivation of Oxide layers of the metals.
Explanation:
Passivation is a non-electrolytic finishing process that makes most metals rust-resistant. The prosses removes free iron from the surface by using either nitric or citric acid. When this happens, it results to an inert, protective oxide layer that is very slow or less likely to chemically react with air and cause corrosion.
Passivity caused many of the metals several minutes to begin to react. Once the finishing process that makes metals less likely to react was eroded, reaction was initiated vigorously.
Answer:
The master mix contains the following reagents: dNTPs, DNA Polymerase, PCR buffer and MgCl2.
Explanation:
The DNA templates are the gene fragments to amplify by PCR, thereby they have to be added separately in each tube. Moreover, the primer pairs are specific for each gene, thereby they have to be added separately in each tube.
Deoxynucleotide triphosphates (dNTPs) are the building blocks of the DNA molecules: dGTP, dATP, TTP, and dCTP.
The PCR buffer provides a suitable medium for the activity of the DNA polymerase, often it contains Tris-Hcl and KCl.
MgCl2 is a cofactor for the activity of the DNA Polymerase.
The DNA Polymerase is an enzyme that amplifies DNA by adding nucleotides to the 3' end.
Answer:
The work for the given process is (- 2263.4 J)
Explanation:
Given: Mass of nitrogen gas (N₂): w = 92 g, external pressure: P = 1 atm, Initial temperature: T₁ = 200 K, Final temperature: T₂ = 200 + 83 K = 283 K
Molar mass of N₂ gas: m = 28 g, Gas constant: R = 8.314 J.K⁻¹.mol⁻¹
The number of moles of N₂ gas = w ÷ m = 92 g ÷ 28 g/mol = 3.28 mole
<u>To find the initial volume (V₁) and final volume (V₂), we use the </u><u>ideal gas equation</u><u>:</u>

<u>So the </u><u>Work</u>:



<u>Therefore, the work for the given process: W = (- 2263.4 J)</u>
Answer:
AB2
Explanation:
The following data were obtained from the question:
Mass of element A = 0.444 g
Molar mass of element A = 111 g/mol
Mass of the compound = 0.988 g
Molar mass of Element B = 68 g/mol
Next, we shall determine the mass of element B. This is shown below:
Mass of element B = Mass of the compound – Mass of Element A
Mass of element B = 0.988 – 0.444
Mass of element B = 0.544 g
Now, we can obtain the empirical formula for the compound formed as follow:
A = 0.444
B = 0.544
Divide by their molar mass.
A = 0.444/111 = 4×10¯³
B = 0.544/68 = 8×10¯³
Divide by the smallest
A = 4×10¯³ /4×10¯³ = 1
B = 8×10¯³/4×10¯³ = 2
Therefore, the empirical formula for the compound formed is AB2