How many g are in 6.35 x 10^31 particles of nickel (Ni) if nickel’s molar mass is 58.693 g/mol?
A. 1.08 x 10^30 g Ni
B. 6.51 x 10^53 g Ni
C. 1.80 x 10^6 g Ni
D. 6.19 x 10^9 g Ni
Waht is 6.35 x 10^31 divided by avag number, all times 58.693? This one actually has a right answer listed
is it b?
No, I told you how to calculate it.
Sorry i put the wrong number for Avagrado's number... It is D right
Yes, correct
To determine the number of grams (g) in a given amount of particles, we can use the concept of molar mass and Avogadro's number.
First, we need to find the number of moles (n) of nickel (Ni) in 6.35 x 10^31 particles. To do this, we can divide the given number of particles by Avogadro's number, which is approximately 6.022 x 10^23 particles/mol.
n = (6.35 x 10^31 particles) / (6.022 x 10^23 particles/mol)
After simplifying:
n ≈ 1.055 x 10^8 mol
Next, we can use the molar mass of nickel (Ni) to find the mass in grams.
Mass (m) = molar mass (M) x moles (n)
m = (58.693 g/mol) x (1.055 x 10^8 mol)
After performing the calculation:
m ≈ 6.14 x 10^9 g Ni
Therefore, the correct answer is option D: 6.19 x 10^9 g Ni.
Note: The decimal place may vary slightly due to rounding during the calculations, so the answer may be listed slightly differently in different sources or answer choices.