Final answer:
To find the pressure of the oxygen gas produced in the sealed container, we can use the ideal gas law equation PV = nRT. By applying this equation and given the given values, we can calculate the pressure of the oxygen gas as 95.43 atm.
Step-by-step explanation:
To find the pressure of the oxygen gas produced, we can use the ideal gas law equation, which is PV = nRT. We can rearrange the equation to solve for pressure by dividing both sides by volume, giving us P = (nRT)/V.
Given that the temperature is 500 K, we can convert it to Celsius by subtracting 273, which gives us 227 °C.
We convert this temperature to Kelvin by adding 273, which gives us 500 K.
The volume is given as 250 milliliters, which we convert to liters by dividing by 1000, giving us 0.25 liters. The number of moles (n) can be calculated by dividing the mass of hydrogen peroxide by its molar mass.
The molar mass of hydrogen peroxide is 34.0147 g/mol.
Therefore, the number of moles (n) is 4.000 g / 34.0147 g/mol = 0.1175 mol.
Plugging in these values into the equation, we get P = (0.1175 mol * 0.0821 L·atm/(mol·K) * 500 K) / 0.25 L
= 95.43 atm.