2.01214904 × 10²² silver atoms are there in 3.74 g of silver
The most common isotope of silver has 60 neutrons, 47 protons, and 47 electrons. Silver is a soft metal with a glossy metallic luster under normal circumstances. It is exceedingly malleable and ductile (can be formed into a wire).
The molar mass of silver is as follows:
Molar mass of Ag = 107.8682 g/mol
The number of atoms in a molar mass is Avogadro’s number:
6.022140857 × 10²³
Therefore 3.8 g of silver contains 3.8 times 6.022140857 × 10²³ divided by 107.8682 that equals 0.03522818 times
6.022140857 × 10²³
= 2.01214904 × 10²² atoms.
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Ratio of neutrons to protons and <span>number of electrons in the outer shell</span>
The molarity of the solution is equal to 0.500M.
<h3>Mole calculation</h3>
To calculate the molarity of a solution, one must use the value of the amount of moles and the volume, so that:
So, applying the values given in the question we have:
So, the molarity of the solution is equal to 0.500M.
Learn more about mole calculation in: brainly.com/question/2845237
Answer:
N2(g) + 3H2(g) → 2 NH3(g)
Explanation:
N2(g) + H2(g) → NH3(g)
We start equaling the number of N atoms in both sides multiplying by 2 the NH3.
N2(g) + H2(g) → 2 NH3(g)
So we equals the H atoms (there are six in products sites)
N2(g) + 3 H2(g) → 2 NH3(g)