What is the molar mass of carbon monoxide (CO)? Atomic weight of carbon is 12 and oxygen is 16. Answer: g/mol How many moles of CO gas if its mass is 65g? Answer: moles How many CO molecules are there in 65g of CO? Answer: x1024 molecules
The Correct Answer and Explanation is:
Answers:
- Molar mass of CO = 12 (C) + 16 (O) = 28 g/mol
- Moles of CO in 65g = 65 g28 g/mol\frac{65 \text{ g}}{28 \text{ g/mol}}28 g/mol65 g = 2.32 moles
- Number of molecules in 65g CO = 2.32×6.022×10232.32 \times 6.022 \times 10^{23}2.32×6.022×1023 ≈ 1.40 × 10²⁴ molecules
Explanation
Carbon monoxide (CO) is a compound consisting of one carbon atom and one oxygen atom. To calculate its molar mass, we sum the atomic weights of its elements. The atomic weight of carbon is 12 g/mol and that of oxygen is 16 g/mol. Therefore, the molar mass of CO is: Molar mass of CO=12+16=28 g/mol\text{Molar mass of CO} = 12 + 16 = 28 \text{ g/mol}Molar mass of CO=12+16=28 g/mol
This means one mole of CO weighs 28 grams.
To determine how many moles are present in 65 grams of CO, we use the formula: Moles=Given massMolar mass=6528≈2.32 moles\text{Moles} = \frac{\text{Given mass}}{\text{Molar mass}} = \frac{65}{28} \approx 2.32 \text{ moles}Moles=Molar massGiven mass=2865≈2.32 moles
Moles are a measure of the number of particles (in this case, CO molecules). One mole contains Avogadro’s number of particles, which is approximately: 6.022×1023 particles/mole6.022 \times 10^{23} \text{ particles/mole}6.022×1023 particles/mole
To find the number of CO molecules in 65 grams, we multiply the number of moles by Avogadro’s number: Number of molecules=2.32×6.022×1023≈1.40×1024 molecules\text{Number of molecules} = 2.32 \times 6.022 \times 10^{23} \approx 1.40 \times 10^{24} \text{ molecules}Number of molecules=2.32×6.022×1023≈1.40×1024 molecules
This large number reflects how many individual CO molecules exist even in relatively small masses of a substance. Understanding these conversions is fundamental in chemistry for analyzing reactions, predicting yields, and working with gases under different conditions.
