If 2.33 L of propane (C3H8) at 24oC and 67.2 kPa is completely burned in excess oxygen, how many moles of carbon dioxide will be produced?

a. Write a balanced equation for the reaction.
b. Use stoichiometry to find the volume of carbon dioxide.
c. Use the ideal gas law to solve the number of moles of propane.

C3H8 + 5O2 ==> 3CO2 + 4H2O

Use PV = nRT and solve for n = number of mols C3H8

Using the coefficients in the balanced equation, convert mols C3H8 to mols of CO2.

I have no clue how to do b and c.

a. The balanced equation for the combustion of propane is:

C3H8 + 5O2 -> 3CO2 + 4H2O

b. To find the volume of carbon dioxide produced, we can use stoichiometry. Let's start by calculating the number of moles of propane:

PV = nRT

where P = pressure (67.2 kPa), V = volume (2.33 L), n = number of moles, R = ideal gas constant (0.0821 L·atm/mol·K), and T = temperature in Kelvin (24°C = 24 + 273 = 297 K).

Rearranging the equation:

n = PV / RT

Substituting the given values:

n = (67.2 kPa * 2.33 L) / (0.0821 L·atm/mol·K * 297 K)

Calculate the value of n.

c. Since the balanced equation tells us that the stoichiometric ratio between propane and carbon dioxide is 1:3, we can say that for every 1 mole of propane burned, 3 moles of carbon dioxide will be produced.

So, multiply the number of moles of propane calculated in part b by 3 to get the number of moles of carbon dioxide.

a. To write a balanced equation for the combustion of propane, we need to know that propane reacts with oxygen to produce carbon dioxide and water vapor. The balanced equation is as follows:

C3H8 + 5O2 -> 3CO2 + 4H2O

b. To find the volume of carbon dioxide produced, we need to use stoichiometry. From the balanced equation, we can see that 1 mole of propane produces 3 moles of carbon dioxide. Therefore, we need to convert the given volume of propane to moles, and then multiply by the mole ratio of carbon dioxide to propane.

To convert the given volume of propane to moles, we use the ideal gas law. The ideal gas law is given by 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.

First, we need to convert the given temperature from Celsius to Kelvin. We add 273.15 to the given temperature to get:

24 oC + 273.15 = 297.15 K

Next, we can arrange the ideal gas law to solve for the number of moles (n) of propane:

n = PV / RT

Given that the pressure (P) is 67.2 kPa, the volume (V) is 2.33 L, the gas constant (R) is 8.314 J/(mol·K), and the temperature (T) is 297.15 K, we can substitute these values into the equation to find the number of moles of propane.

c. Now that we have the number of moles of propane, we can multiply it by the mole ratio of carbon dioxide to propane to find the number of moles of carbon dioxide produced. From the balanced equation, we know that 1 mole of propane produces 3 moles of carbon dioxide.

So, to find the number of moles of carbon dioxide, we can multiply the number of moles of propane by the mole ratio of 3 moles of CO2 per 1 mole of C3H8.

Finally, we have the number of moles of carbon dioxide produced.