2C2H6(g)+7O2(g)--> 4Co2 (g)+6H2O(l)
A) if 3.00 moles of C2H6 and 9.00 moles of O2 are introducedinto an empty container at 32.0 degree C and then ignited tointiate the above reaction calculate the mass of water that isproduced.
B) if the container volume is 675 what mass of water is in thevapour phase?
Convert 3.00 C2H6 to mols H2O. That's 3.00 x (6 mol H2O/2 mols C2H6) = 9.00 mols H2O
Do the same for mols O2 to mols H2O. That's 9.00 x (6 mols H2O/7 mols O2) = 7.71 mols H2O.
In limiting reagent problems the smaller number is ALWAyS the correct choice; therefore, O2 is the limiting reagent and 7.71 mols H2O will be formed. Then g H2O = mols H2O x molar mass H2O = ?
B. That's 675 what? mL? L?
Look up the vapor pressure H2O @ 32 C, plug all of the numbers into PV = nRT and solve for n. Then n = grams/molar mass. You know n and molar mass, solve for mass H2O in the vapor phase.
To answer these questions, we need to use stoichiometry and the concept of mole ratios.
A) To calculate the mass of water produced, we need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed and determines the maximum amount of product formed.
1. Calculate the amount of CO2 produced: Since the balanced equation shows that 2 moles of C2H6 produce 4 moles of CO2, and we have 3 moles of C2H6, we can use the following proportion: (4 moles CO2 / 2 moles C2H6) * 3 moles C2H6 = 6 moles CO2.
2. Calculate the amount of H2O produced: Since the balanced equation shows that 2 moles of C2H6 produce 6 moles of H2O, and we have 3 moles of C2H6, we can use the following proportion: (6 moles H2O / 2 moles C2H6) * 3 moles C2H6 = 9 moles H2O.
3. Calculate the molar mass of H2O: H2O consists of 2 hydrogen atoms (2 g/mol each) and 1 oxygen atom (16 g/mol), so the molar mass of H2O is 2 * 1 + 16 = 18 g/mol.
4. Calculate the mass of H2O: Multiply the molar mass of H2O by the moles of H2O calculated in step 2: 18 g/mol * 9 moles H2O = 162 g H2O.
Therefore, the mass of water produced is 162 grams.
B) To calculate the mass of water in the vapor phase, we need to determine the number of moles of water vapor present. To do this, we need to know the pressure of the system as well as the temperature.
Since the temperature is given as 32.0 degrees Celsius, we need to convert it to Kelvin by adding 273.15: T = 32.0 + 273.15 = 305.15 K.
Using the ideal gas law equation 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:
1. Calculate the number of moles of water vapor: We know the volume of the container (675 L) and the temperature (305.15 K). We also need to know the pressure of the system to use the ideal gas law equation.
2. Once we know the number of moles of water vapor, we can calculate the mass of water using its molar mass (18 g/mol).
Please provide the pressure of the system to continue with the calculation.