Stainless steel is an alloy of iron containing 5 percent nickel and 0.

175 percent chromium. How much chromium is present in a 72.2 g
sample of this alloy? Answer in units of mol.

g Cr present = 0.175 x 72.2 = ?

Then mols = grams/atomic mass.

To calculate the amount of chromium present in the alloy, we need to find the number of moles of chromium in the sample.

To do this, we can use the molar mass of chromium. The molar mass of chromium is 52 g/mol.

First, let's calculate the mass of chromium in the sample:
Mass of chromium = (0.175 / 100) * 72.2 g = 0.12635 g

Now, we will convert the mass of chromium to moles:
Number of moles of chromium = Mass of chromium / Molar mass of chromium
Number of moles of chromium = 0.12635 g / 52 g/mol

Calculating this value gives us:
Number of moles of chromium ≈ 0.00243 mol

Therefore, there is approximately 0.00243 mol of chromium present in the 72.2 g sample of the alloy.

To determine the amount of chromium present in the alloy, we need to convert the given mass of the sample to moles.

First, let's calculate the molar mass of the alloy.

The molar mass of 1 mole of stainless steel can be calculated as follows:

(Molar mass of iron × Percentage of iron) +
(Molar mass of nickel × Percentage of nickel) +
(Molar mass of chromium × Percentage of chromium)

The molar mass of iron (Fe) is approximately 55.85 g/mol, the molar mass of nickel (Ni) is approximately 58.69 g/mol, and the molar mass of chromium (Cr) is approximately 52.00 g/mol.

Let's substitute these values into the equation:

Molar mass = (55.85 × Percentage of iron) + (58.69 × Percentage of nickel) + (52.00 × Percentage of chromium)
= (55.85 × 1) + (58.69 × 0.05) + (52.00 × 0.00175)
= 55.85 + 2.9345 + 0.091

Now, let's calculate the moles of the sample:

Moles = Mass of sample / Molar mass
= 72.2 g / Molar mass

Substituting the calculated molar mass into the equation:

Moles = 72.2 g / (55.85 + 2.9345 + 0.091)

Now, we can calculate the moles of chromium present:

Moles of Chromium = Moles of sample × Percentage of chromium
= Moles × 0.0175

Substituting the value of moles into the equation:

Moles of Chromium = (72.2 g / (55.85 + 2.9345 + 0.091)) × 0.0175

Evalutating the expression, we get:

Moles of Chromium ≈ 0.0146 mol

Therefore, the amount of chromium present in the 72.2 g sample of the alloy is approximately 0.0146 mol.