Calculate the grams of oxygen gas present in 2.5 L sample kept at 1.66 atm pressure and a temperature of 10 C.
- I got 5.72 grams
Determine the volume of oxygen gas needed to completely combust 0.202 L of Butane(C4H10).
-I got 1.31 L O2.
-Thanks
To calculate the grams of oxygen gas present in a given sample, you need to use the ideal gas law equation, which relates the pressure (P), volume (V), temperature (T), and the number of moles of a gas (n). The ideal gas law equation is as follows:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L*atm/(mol*K))
T = temperature (in Kelvin)
First, let's convert the given values to the appropriate units:
Pressure: 1.66 atm
Volume: 2.5 L
Temperature: 10°C (to convert to Kelvin, add 273.15) => 10°C + 273.15 = 283.15 K
Now, we can plug in the values into the ideal gas law equation:
PV = nRT
(1.66 atm)(2.5 L) = n(0.0821 L*atm/(mol*K))(283.15 K)
You can cross multiply and solve for n:
n = (1.66 atm * 2.5 L) / (0.0821 L*atm/(mol*K) * 283.15 K)
n ≈ 0.243 moles
To determine the grams of oxygen gas, we need to use the molar mass of oxygen, which is 32 g/mol. You can now calculate the grams using the formula:
grams = moles * molar mass
grams = 0.243 moles * 32 g/mol
grams ≈ 7.78 grams
Therefore, the correct value for the grams of oxygen gas in the 2.5 L sample is approximately 7.78 grams, not 5.72 grams.
For the second question, to determine the volume of oxygen gas needed to completely combust butane (C4H10), we need to know the balanced chemical equation for the combustion of butane, which is:
2 C4H10 + 13 O2 → 8 CO2 + 10 H2O
From the balanced equation, we can see that the ratio of oxygen to butane is 13:2. So, for every 13 moles of oxygen, we need 2 moles of butane.
Given that you have 0.202 L of butane, you'll need to calculate the number of moles. However, the temperature and pressure of the butane are not provided, and they are required for accurate calculations using the ideal gas law. Could you please provide the pressure and temperature of the butane for an accurate calculation of the moles?