One molecule of the protein myoglobin contains one atom of iron. A myoglobinsample was found to contain 0.34% iron. The molecular weight of myoglobinis __________ 𝑔 𝑚𝑜𝑙−1 (rounded off to the nearest integer).(Use 55.9 𝑔 𝑚𝑜𝑙−1 as atomic mass of iron)

To solve this problem, we need to find the molecular weight of myoglobin. We know that myoglobin contains 0.34% iron by weight, and that one molecule of myoglobin contains one atom of iron.

Step 1: Convert the percentage of iron to a decimal. 0.34% = 0.0034

Step 2: We know that the atomic mass of iron is 55.9 g/mol. Since there is one atom of iron in each molecule of myoglobin, the weight of iron in each molecule of myoglobin is also 55.9 g/mol.

Step 3: Now, we can set up a proportion to find the molecular weight of myoglobin. If 55.9 g/mol is 0.0034 of the total weight, we can set up the following equation:

55.9 g/mol / X g/mol = 0.0034 / 1

Step 4: Solve for X. X = 55.9 g/mol / 0.0034 = 16441.18 g/mol

Step 5: Round to the nearest integer. The molecular weight of myoglobin is approximately 16441 g/mol.