How do you solve this: if 24.0 L of O2 burns completely a sample of carbon disulfide, how many grams of sulfur dioxide will be produced at 15 degrees celcius at a pressure of 1.3 atm? (the answer is 45.7 g).
CS2 + 3CO2 -> CO2 + 2SO2
I am assuming you meant 24.0L of CO2 not O2.
Use the following formula:
PV=nRT
Where
P=1.3 atm
V=24.0L
n=?
R=0.08205746
T=273.15 + 15=288.15 K
Solve for moles of O2
moles of CO2=n=PV/RT
******1 moles of CO2=2 moles of SO2
moles of CO2*(2 moles of SO2/1 mole of CO2)= moles of SO2
moles of SO2*(64.066 g/mol)= mass of SO2
I made a typo,
it should say
******3 moles of CO2=2 moles of SO2
moles of CO2*(2 moles of SO2/3 mole of CO2)= moles of SO2
moles of SO2*(64.066 g/mol)= mass of SO2
But when I punch in the numbers I am not getting 45.7g but I am getting about 56 g. So, I am not sure about this problem.
the equation is supposed to say:
CS2 + 3O2 -> CO2 + 2SO2
* O2 not 3CO2
Still doesn't change my overall answer.
To solve this problem, you need to use stoichiometry, which involves converting between the given quantities and the desired quantity using the balanced chemical equation. Here's how to solve it step by step:
Step 1: Write and balance the chemical equation:
CS2 + 3O2 -> CO2 + 2SO2
Step 2: Calculate the number of moles of O2:
Number of moles of O2 = volume (L) / molar volume (L/mol)
Number of moles of O2 = 24.0 L / 22.4 L/mol (at STP)
Number of moles of O2 = 1.071 mol
Step 3: Use the stoichiometry of the balanced equation to convert from moles of O2 to moles of SO2:
From the balanced equation, the stoichiometry is: 1 mol O2 produces 2 mol SO2
Number of moles of SO2 = 1.071 mol O2 * (2 mol SO2 / 1 mol O2)
Number of moles of SO2 = 2.142 mol SO2
Step 4: Convert the moles of SO2 to grams using the molar mass of SO2:
Molar mass of SO2 = 32.07 g/mol (atomic masses: S = 32.06 g/mol, O = 16.00 g/mol)
Mass of SO2 = 2.142 mol SO2 * 32.07 g/mol
Mass of SO2 = 68.6 g
However, this calculation is for STP (Standard Temperature and Pressure) conditions. To account for the given temperature and pressure (15 degrees Celsius and 1.3 atm), we need to use the ideal gas law.
Step 5: Convert the given temperature to Kelvin:
Temperature in Kelvin = 15 degrees Celsius + 273.15
Temperature in Kelvin = 288.15 K
Step 6: Use the ideal gas law, PV = nRT, to calculate moles of O2:
n = PV / RT, where P is pressure, V is volume, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is temperature.
n = (1.3 atm) * (24.0 L) / (0.0821 L·atm/(mol·K) * 288.15 K)
n = 1.071 mol (rounded to three decimal places)
Step 7: Repeat steps 3 and 4 to find the actual number of moles and mass of SO2:
Number of moles of SO2 = 1.071 mol O2 * (2 mol SO2 / 1 mol O2)
Number of moles of SO2 = 2.142 mol SO2
Mass of SO2 = 2.142 mol SO2 * 32.07 g/mol
Mass of SO2 = 68.8 g (rounded to one decimal place)
Therefore, the correct answer is approximately 68.8 g at the given conditions, not 45.7 g as stated in your question.