Consider the combustion of nitrogen monoxide:
NO(g) + ½ O2(g) NO2 (g) ΔH = -56.5 kJ/mol
How much heat would be released by the combustion of 65 g of NO (g)?
I'm so stuck please help
N + O = 14 + 16 = 30 grams / mol
65 / 30 = 0.2 mols of NO
multiply by the Kilojoules / mol
Ah, combustion reactions can be quite hot! But fear not, my friend, Clown Bot is here to help, with jokes hotter than any reaction!
To calculate the heat released, we need to use the molar mass of NO (g) to convert 65 g into moles. The molar mass of NO is approximately 30 g/mol. So, 65 g of NO would be about 2.17 moles (65 g divided by 30 g/mol).
Now, to calculate the heat released, we multiply the moles of NO by the value of ΔH, which is -56.5 kJ/mol. So, it would be:
2.17 moles × (-56.5 kJ/mol) = -122.305 kJ
So, approximately -122.305 kJ of heat would be released during the combustion of 65 g of NO. That's quite a fiery reaction! Remember, negative values indicate heat release. Keep that fire extinguisher handy!
To calculate the heat released by the combustion of NO(g), we need to use the given enthalpy change value and the molar mass of NO.
1. Find the molar mass of NO:
The molar mass of nitrogen (N) is approximately 14.01 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol. Since NO consists of one nitrogen atom and one oxygen atom, the molar mass of NO is:
Molar mass of NO = Molar mass of N + Molar mass of O
Molar mass of NO = 14.01 g/mol + 16.00 g/mol
Molar mass of NO = 30.01 g/mol
2. Calculate the number of moles of NO:
To find the number of moles, divide the given mass of NO by its molar mass:
Number of moles of NO = Mass of NO / Molar mass of NO
Number of moles of NO = 65 g / 30.01 g/mol
Number of moles of NO ≈ 2.1668 mol (rounded to four decimal places)
3. Calculate the heat released:
Since the enthalpy change value is given per mole, we can multiply it by the number of moles to find the heat released:
Heat released = ΔH × Number of moles of NO
Heat released = -56.5 kJ/mol × 2.1668 mol
Heat released ≈ -122.47 kJ (rounded to two decimal places)
Therefore, approximately -122.47 kJ of heat would be released by the combustion of 65 g of NO(g). The negative sign indicates that the process is exothermic (heat is released).
To calculate the amount of heat released in the combustion of nitrogen monoxide (NO), you need to use the given value of enthalpy change (ΔH) and the molar mass of NO.
First, let's find the number of moles of NO. We can do this by dividing the given mass of NO (65 g) by the molar mass of NO.
The molar mass of NO can be calculated by adding the atomic masses of nitrogen (N) and oxygen (O):
Molecular mass of NO = atomic mass of N + atomic mass of O
= (14.01 g/mol) + (16.00 g/mol)
= 30.01 g/mol
Now, let's calculate the number of moles of NO:
Number of moles = mass / molar mass
= 65 g / 30.01 g/mol
≈ 2.166 moles
Next, we need to use the stoichiometric coefficients from the balanced equation to determine the heat released per mole of NO combusted. From the balanced equation, we see that the stoichiometric coefficient of NO is 1, meaning that 1 mole of NO will produce -56.5 kJ of heat.
Finally, we can calculate the total heat released by multiplying the number of moles of NO by the enthalpy change per mole:
Total heat released = number of moles × enthalpy change per mole
= 2.166 moles × -56.5 kJ/mol
≈ -122.37 kJ
The negative sign indicates that heat is being released in the combustion reaction.
Therefore, the combustion of 65 g of nitrogen monoxide (NO) would release approximately -122.37 kJ of heat.