A reaction between liquid reactants takes place at −5.0°C in a sealed, evacuated vessel with a measured volume of 5.0L. Measurements show that the reaction produced 15.g of dinitrogen difluoride gas.Calculate the pressure of dinitrogen difluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.
Question
A reaction between liquid reactants takes place at −5.0°C in a sealed, evacuated vessel with a measured volume of 5.0L. Measurements show that the reaction produced 15.g of dinitrogen difluoride gas.Calculate the pressure of dinitrogen difluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.
Solution
To solve this problem, we need to use the ideal gas law equation, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Step 1: Convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, -5.0°C = -5.0 + 273.15 = 268.15 K.
Step 2: Calculate the number of moles of dinitrogen difluoride. The molar mass of dinitrogen difluoride (N2F2) is approximately 104 g/mol. So, 15 g of N2F2 is 15 g / 104 g/mol = 0.144 moles.
Step 3: Substitute the values into the ideal gas law equation. The ideal gas constant R can be taken as 0.0821 L·atm/(mol·K) for this calculation. So, P = nRT/V = (0.144 mol * 0.0821 L·atm/(mol·K) * 268.15 K) / 5.0 L = 0.64 atm.
So, the pressure of dinitrogen difluoride gas in the reaction vessel after the reaction is approximately 0.64 atm.
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