Calculate the volume of oxygen you would need, at 1.00 atm \rm atm and 298 K \rm K, to completely oxidize 50g g of glucose
To calculate the volume of oxygen needed to completely oxidize 50g of glucose, we need to follow the following steps:
Step 1: Write the balanced equation for the combustion of glucose.
The balanced equation for the combustion of glucose is:
C6H12O6 + 6O2 -> 6CO2 + 6H2O
Step 2: Calculate the number of moles of glucose.
To calculate the number of moles, we divide the given mass of glucose (50g) by the molar mass of glucose (180.16g/mol).
Number of moles of glucose = 50g / 180.16g/mol
Step 3: Determine the stoichiometric ratio.
From the balanced equation, we can see that the stoichiometric ratio between glucose and oxygen is 1:6. This means that for every mole of glucose, we need 6 moles of oxygen.
Step 4: Calculate the number of moles of oxygen.
Number of moles of oxygen = Number of moles of glucose x 6
Step 5: Use the ideal gas law to calculate the volume of oxygen.
The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
To calculate the volume of oxygen, we need to rearrange the equation as follows:
V = (nRT) / P
Given:
Pressure (P) = 1.00 atm
Temperature (T) = 298 K
Number of moles of oxygen (n) = calculated in Step 4
Step 6: Calculate the volume of oxygen.
Substitute the values into the equation and calculate:
V = (number of moles of oxygen x gas constant x temperature) / pressure
Make sure to use the appropriate units for the gas constant (R) depending on the units chosen for pressure (P) and temperature (T). The value of the gas constant varies depending on the unit system being used.
After performing the calculation, you will have the volume of oxygen needed to completely oxidize 50g of glucose at 1.00 atm and 298 K.
write the balanced equation.
Secondly, determine the moles of 50g of glucose. Then, using the mole ratio of glucose/oxygen, how many moles of O2 do you need?
convert that moles to volume, using
PV=nRT