Consider the combustion of propane:

C3H8(g)+5O2(g) yields 3CO2(g) + 4H2O(l)
delta H= -2221 kJ
Assume that all of the heat comes from the combustion of propane. Calculate delta H in which 5.00g of propane is burned in excess oxygen at constant pressure.

Find the number moles and of is equal to 0.1136mol

then multiply the delta H=-2221KJ
finally the answer is equal to -252.3KJ

-252.4

Well, let me first say that I admire the combustion of propane for always finding a way to heat things up. Now, to calculate the enthalpy change, delta H, let's use some good old math.

We're given that the enthalpy change for the combustion of propane is -2221 kJ. This means that when 1 mole of propane is burned, -2221 kJ of heat is released.

To calculate the enthalpy change for 5.00g of propane, we need to convert grams to moles. The molar mass of propane (C3H8) is about 44.1 g/mol.

So, 5.00g of propane is equal to 5.00g / 44.1 g/mol ≈ 0.113 mol.

Since the ratio of propane to enthalpy change is 1:1, we can simply multiply the number of moles of propane by the enthalpy change, like so:

delta H = -2221 kJ/mol * 0.113 mol ≈ -251 kJ

Therefore, the enthalpy change for burning 5.00g of propane is approximately -251 kJ. And just like that, propane brings the heat once again!

To calculate the ΔH (enthalpy change) in which 5.00g of propane is burned, you need to use the given ΔH value (-2221 kJ) and the molar mass of propane (C3H8) to determine the amount of propane being burned.

1. Calculate the molar mass of propane (C3H8):
- Carbon (C) has a molar mass of 12.01 g/mol, and there are 3 carbon atoms in propane.
- Hydrogen (H) has a molar mass of 1.01 g/mol, and there are 8 hydrogen atoms in propane.
- Multiply the molar mass of carbon by 3 and the molar mass of hydrogen by 8, then add the results together to get the molar mass of propane:
Molar mass of propane (C3H8) = (3 * 12.01 g/mol) + (8 * 1.01 g/mol)

2. Use the molar mass of propane to calculate the moles of propane in 5.00g:
- Divide the given mass (5.00g) by the molar mass of propane calculated in step 1.

3. Once you have the moles of propane, you can use the balanced equation to determine the relationship between the moles of propane and the enthalpy change:
- According to the balanced equation, 1 mole of propane produces ΔH = -2221 kJ.
- Multiply the moles of propane (calculated in step 2) by the ΔH value to find the enthalpy change for the given amount of propane.

Note: The equation provides the enthalpy change for 1 mole of propane. If you want to calculate the enthalpy change for more or less propane, simply multiply or divide the moles of propane by the ΔH value.

Let's go through the calculations step by step:

1. Molar mass of propane (C3H8):
Molar mass of carbon (C) = 12.01 g/mol
Molar mass of hydrogen (H) = 1.01 g/mol
Molar mass of propane (C3H8) = (3 * 12.01 g/mol) + (8 * 1.01 g/mol)

2. Moles of propane:
Moles of propane = Given mass (5.00g) / Molar mass of propane

3. Enthalpy change:
Enthalpy change = Moles of propane * ΔH

Calculate each step and substitute the values into the equations to find the enthalpy change for the given amount of propane.

-2221 kJ x (5/molar mass C3H8) = ?