How to solve partial pressure given water vapor pressure?

1 answer:

6 0

The partial pressure of water in the mixture, Pwater, is the equilibrium vapour pressure of water at the temperature specified. At 298 K, from the data at the beginning of the questions section, Pwater = 3.17 kPa. Using the Ideal Gas Equation, the number of moles of N2 can be calculated.

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How many grams of oxygen are required to burn 13.5 g of acetylene

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Answer:

41.54 grams of oxygen are required to burn 13.5 g of acetylene

Explanation:

The balanced reaction is:

2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

C₂H₂: 2 moles
O₂: 5 moles
CO₂: 4 moles
H₂O: 2 moles

Being the molar mass of the compounds:

C₂H₂: 26 g/mole
O₂: 32 g/mole
CO₂: 44 g/mole
H₂O: 18 g/mole

By reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

C₂H₂: 2 moles* 26 g/mole= 52 grams
O₂: 5 moles* 32 g/mole= 160 grams
CO₂: 4 moles* 44 g/mole= 176 grams
H₂O: 2 moles* 18 g/mole= 36 grams

You can apply the following rule of three: if by stoichiometry 52 grams of acetylene react with 160 grams of oxygen, 13.5 grams of acetylene react with how much mass of oxygen?

$mass of oxygen=\frac{13.5 grams of acetylene*160 grams of oxygen}{52 grams of acetylene}$