1) What volume of oxygen gas at 28 Celsius and 102 kPa is needed to react completely with 150 g of iron according to the following reaction. Fe(s) + O2 (g) FeO(s)
2) A bunsen burner is lit in a lab that at 24.7 Celcius and 1.07 atm. What mass of water is produced in the complete combustion of 4.5 L of methane gas?
To answer both questions, we need to use the ideal gas law and balanced chemical equations. Let's break down the process step by step:
1) What volume of oxygen gas at 28 Celsius and 102 kPa is needed to react completely with 150 g of iron according to the following reaction: Fe(s) + O2(g) → FeO(s)
a) Balanced Chemical Equation:
The balanced equation shows the stoichiometry of the reaction, indicating the ratio between the reactants and the products. In this case, it is already balanced and tells us that one mole of iron reacts with one mole of oxygen gas to produce one mole of iron(II) oxide (FeO).
b) Calculate the Moles of Iron:
To determine the necessary amount of oxygen gas, we first need to find the moles of iron present in 150 g of iron, using its molar mass. The molar mass of iron (Fe) is 55.845 g/mol.
Moles of Iron = Mass of Iron / Molar Mass of Iron
Moles of Iron = 150 g / 55.845 g/mol
c) Determine the Volume of Oxygen Gas:
Using the ideal gas law, which states PV = nRT (where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature), we can calculate the volume of oxygen gas.
V = nRT / P
V = (Moles of Iron) * (Ideal Gas Constant) * (Temperature in Kelvin) / (Pressure)
However, we need to convert the temperature given in Celsius to Kelvin before using the formula.
Temperature in Kelvin = Temperature in Celsius + 273.15
Once we have the temperature in Kelvin, we can substitute the values into the formula and calculate the volume of oxygen gas required.
2) A Bunsen burner is lit in a lab that is at 24.7 Celsius and 1.07 atm. We need to determine the mass of water produced in the complete combustion of 4.5 L of methane gas.
a) Balanced Chemical Equation:
The complete combustion of methane gas (CH4) yields carbon dioxide (CO2) and water (H2O). The balanced equation is:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
b) Determine the Moles of Methane Gas:
To calculate the moles of methane gas, we will use the ideal gas law formula PV = nRT.
In this case, we are given the volume (V) of methane gas, the pressure (P), and the temperature (T) in Celsius. Like in the previous example, we need to convert the temperature to Kelvin.
c) Determine the Moles of Water:
From the balanced equation, we can see that for every mole of methane gas consumed, two moles of water are produced.
d) Calculate the Mass of Water:
Finally, we need to calculate the mass of water produced from the moles of water using its molar mass. The molar mass of water (H2O) is 18.015 g/mol.
Mass of Water = Moles of Water * Molar Mass of Water
By following these steps and using the appropriate formulas, you can find the answers to both questions.