I NEED HELP ASAP
Here's the problem I'm struggling with: When 1.00 mole of ethlyene (C2H4) is burned at constant pressure, 1410 kJ of energy is released as heat. Calculate delta H for a process in which 10.0 g of ethlyene is burned at constant pressure.
Please show me the specific steps used to find delta H. It doesn't make sense to me, but I'm sure I can understand if someone explains.
To calculate delta H for the given process, you need to follow a few steps.
Step 1: Find the molar mass of ethylene (C2H4).
The molar mass of C2H4 is:
2(12.01 g/mol) + 4(1.01 g/mol) = 28.05 g/mol
Step 2: Calculate the number of moles of ethylene using its mass.
Given that the mass of ethylene is 10.0 g, we can calculate the moles using the equation:
moles = mass / molar mass
moles = 10.0 g / 28.05 g/mol = 0.356 mol
Step 3: Use the given energy change for 1.00 mole of ethylene to find delta H for 0.356 moles.
The energy released in the combustion of one mole (delta H) is 1410 kJ.
Therefore, the energy released for 0.356 moles would be:
1410 kJ/mol * 0.356 mol = 501.96 kJ
So, the value of delta H for the process in which 10.0 g of ethylene is burned at constant pressure is approximately 502 kJ, since we are rounding to three significant figures.
Keep in mind that delta H represents the heat change that occurs at constant pressure. It is often referred to as the enthalpy change of a reaction or process.