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Tell me what explain molecularity what volume will 25.0g of oxygen occupy at 20°c and pressure at0.880 ATM show solving clearly
Accepted Answer
Molecularity:
Molecularity refers to the number of molecules that participate in the rate-determining step of a chemical reaction. It is a theoretical concept that describes the molecularity of a reaction. For example:
Unimolecular reaction: A reaction that involves only one molecule in the rate-determining step (e.g., decomposition of nitrogen pentoxide).
Bimolecular reaction: A reaction involving two molecules in the rate-determining step (e.g., the reaction between hydrogen and iodine).
Termolecular reaction: A reaction involving three molecules in the rate-determining step (these are rare).
Calculating the volume of oxygen:
To solve this, we can use the ideal gas law: PV = nRT, where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
Step 1: Convert temperature to Kelvin:
20°C + 273.15 = 293.15 K
Step 2: Calculate the number of moles (n) of oxygen:
Molar mass of oxygen (O2) = 32 g/mol
n = mass / molar mass = 25.0 g / 32 g/mol = 0.781 mol
Step 3: Substitute the values into the ideal gas law and solve for V:
V = (nRT) / P
V = (0.781 mol
0.0821 L·atm/mol·K
293.15 K) / 0.880 atm
V ≈ 21.6 L
Therefore, 25.0 g of oxygen will occupy approximately 21.6 liters at 20°C and 0.880 atm.
Molecularity refers to the number of molecules that participate in the rate-determining step of a chemical reaction. It is a theoretical concept that describes the molecularity of a reaction. For example:
Unimolecular reaction: A reaction that involves only one molecule in the rate-determining step (e.g., decomposition of nitrogen pentoxide).
Bimolecular reaction: A reaction involving two molecules in the rate-determining step (e.g., the reaction between hydrogen and iodine).
Termolecular reaction: A reaction involving three molecules in the rate-determining step (these are rare).
Calculating the volume of oxygen:
To solve this, we can use the ideal gas law: PV = nRT, where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
Step 1: Convert temperature to Kelvin:
20°C + 273.15 = 293.15 K
Step 2: Calculate the number of moles (n) of oxygen:
Molar mass of oxygen (O2) = 32 g/mol
n = mass / molar mass = 25.0 g / 32 g/mol = 0.781 mol
Step 3: Substitute the values into the ideal gas law and solve for V:
V = (nRT) / P
V = (0.781 mol
0.0821 L·atm/mol·K
293.15 K) / 0.880 atm
V ≈ 21.6 L
Therefore, 25.0 g of oxygen will occupy approximately 21.6 liters at 20°C and 0.880 atm.
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