19.4 g of butane (58.12 g/mol) undergoes combustion according to the following equation. What pressure of carbon dioxide in atm is produced at 309 K in a 1.15 L flask.
2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g)
Balance the equation.
Convert g butane to mols.
Using the coefficients in the balanced equation, convert mols butane to mols CO2.
Use PV = nRT substitute and solve for P of CO2
To find the pressure of carbon dioxide (CO2) produced, we first need to calculate the moles of butane (C4H10) used and the moles of CO2 produced. Then, we can use the ideal gas law equation to find the pressure.
Step 1: Calculate the moles of butane (C4H10) used.
Molar mass of butane (C4H10) = 58.12 g/mol
Given mass of butane = 19.4 g
Moles of butane (C4H10) = mass of butane (C4H10) / molar mass of butane (C4H10)
= 19.4 g / 58.12 g/mol
≈ 0.334 mol
Step 2: Calculate the moles of CO2 produced using the balanced equation.
According to the balanced equation:
2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g)
The ratio between butane (C4H10) and CO2 is 2:8. So, moles of CO2 produced will be 4 times the moles of butane used.
Moles of CO2 = 4 * Moles of butane
= 4 * 0.334 mol
= 1.336 mol
Step 3: Calculate the pressure of CO2 using the ideal gas law equation.
Ideal Gas Law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L atm/mol K)
T = temperature (in K)
Given:
Volume (V) = 1.15 L
Temperature (T) = 309 K
Number of moles (n) of CO2 = 1.336 mol
Ideal gas constant (R) = 0.0821 L atm/mol K
Rearranging the equation, we get:
P = (nRT) / V
Substituting the values:
P = (1.336 mol * 0.0821 L atm/mol K * 309 K) / 1.15 L
≈ 28.23 atm
Therefore, the pressure of carbon dioxide (CO2) produced is approximately 28.23 atm.
To find the pressure of carbon dioxide (CO2) produced in the combustion of butane, you can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in K)
First, we need to calculate the number of moles of butane (C4H10) from the given mass. The molar mass of butane is 58.12 g/mol.
Number of moles = mass / molar mass
Number of moles = 19.4 g / 58.12 g/mol
Next, let's calculate the number of moles of carbon dioxide (CO2) produced using the stoichiometric coefficients from the balanced equation. According to the equation, 2 moles of butane produce 8 moles of CO2.
Number of moles of CO2 = (number of moles of butane) * (moles of CO2 / moles of butane)
Number of moles of CO2 = (19.4 g / 58.12 g/mol) * (8 mol CO2 / 2 mol butane)
Now, we can substitute the values into the ideal gas law equation to find the pressure of CO2:
P * V = n * R * T
P * (1.15 L) = [(19.4 g / 58.12 g/mol) * (8 mol CO2 / 2 mol butane)] * (0.0821 L·atm/mol·K) * (309 K)
Simplifying the equation, we get:
P = [(19.4 g / 58.12 g/mol) * (8 mol CO2 / 2 mol butane)] * (0.0821 L·atm/mol·K) * (309 K) / (1.15 L)
Now, let's calculate the pressure of carbon dioxide using this equation.