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The vapour density of carbon dioxide is ...

The vapour density of carbon dioxide is 22. What is its gram molecular mass?

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To find the gram molecular mass of carbon dioxide (CO₂) given its vapor density, we can follow these steps: ### Step-by-Step Solution: 1. **Understand the Definition of Vapor Density**: - Vapor density (Vd) is defined as the density of a gas relative to the density of hydrogen. It can be expressed as: \[ \text{Vapor Density} = \frac{\text{Molecular Mass of the Gas}}{\text{Molecular Mass of Hydrogen}} ...
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ICSE-MOLE CONCEPT AND STOICHIOMETRY-IMPORTANT NUMERICAL EXERCISES
  1. How many molecules are there in 22.4 L of H(2) at STP?

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  2. What is the mass of 11.2 L of N(2) at STP?

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  3. The vapour density of carbon dioxide is 22. What is its gram molecular...

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  4. Atomic mass of chlorine is 35.5. What is its vapour density?

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  5. Which one in each of the following sets will occupy more volume at STP...

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  6. Which one in each of the following sets will occupy more volume at STP...

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  7. Which one in each of the following sets will occupy more volume at STP...

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  8. Which one in each of the following sets will occupy more volume at STP...

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  9. Calculate the mass of each of the following at STP: 5.6L O(2)

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  10. Calculate the mass of each of the following at STP: 11.2 L CO(2)

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  11. Calculate the mass of each of the following at STP: 5.6 L N(2)

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  12. Calculate the mass of each of the following at STP: 22.4 L H(2)

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  13. Calculate the mass of each of the following at STP: 112 LCl(2)

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  14. Calculate the volume occupied by 15 g of a gas at STP. Its relative mo...

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  15. What is the volume of 7.1 g Cl(2) at STP?

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  16. Calculate the ratio of the number of molecules in 2 L of oxygen and 8 ...

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  17. Find the ratio of the number of moles in 2 g of oxygen and 8 g nitroge...

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  18. The ratio of the mass of a sulphur atom to that of an oxygen atom is 2...

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  19. Compute the number of O atoms in 54 g of water. M(H(2)O) = 18 g.

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  20. A vessel contains 5.6 g of nitrogen (N(2)) gas. Calculate the followin...

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