Determine the amount of heat (in kJ) given off when 1.26 x 104 g of NO2 are produced according to the equation:

2NO(g)  +  O2(g)  →  2NO2(g)       ΔH = -114.6 kJ/mol

According to the equation you get 114.6 kJ/mol or 229.2 kJ/2 mols or 222.9 kJ/92 g so use that as your conversion factor as follows:

222.9 kJ x (12600 g/92 g) = ?

oops. I transposed some numbers. The following should fix that.

According to the equation you get 114.6 kJ/mol or 229.2 kJ/2 mols or 229.2 kJ/92 g so use that as your conversion factor as follows:
229.2 kJ x (12600 g/92 g) = ?

Determine the amount of heat (in kJ) given off when 1.26 3 10 4 g of NO 2 are 2NO(g)+O2(g) to 2NO2(g)

Well, let's do some chemistry math! First, we need to figure out the number of moles of NO2 produced. Since the equation tells us that 2 moles of NO2 are produced per 2 moles of NO, we can conclude that the number of moles of NO2 produced is the same as the number of moles of NO.

To find the number of moles of NO, we divide the mass of NO by its molar mass. The molar mass of NO is 30.01 g/mol, so:

Moles of NO = (1.26 x 10^4 g) / (30.01 g/mol)

Now, we need to calculate the heat released using the molar value of NO2. The equation gives us a molar value of -114.6 kJ/mol. Since the number of moles of NO2 is the same as the number of moles of NO:

Heat released = -114.6 kJ/mol x (1.26 x 10^4 g) / (30.01 g/mol)

After doing the calculation, we get the amount of heat released when 1.26 x 10^4 g of NO2 are produced.

To determine the amount of heat (in kJ) given off when 1.26 x 10^4 g of NO2 is produced, we need to follow these steps:

Step 1: Find the molar mass of NO2. The molar mass of NO2 can be calculated by adding the atomic masses of nitrogen (N) and two oxygen (O) atoms together. The atomic mass of nitrogen is 14.01 g/mol, and the atomic mass of oxygen is 16.00 g/mol. Therefore, the molar mass of NO2 is 14.01 g/mol + 2 * 16.00 g/mol = 46.01 g/mol.

Step 2: Convert the given mass of NO2 into moles. We can use the molar mass of NO2 calculated in step 1 to convert grams into moles. The formula to convert grams to moles is:
moles = mass / molar mass.

In this case, moles = 1.26 x 10^4 g / 46.01 g/mol = 274.3 mol.

Step 3: Use the stoichiometry of the balanced chemical equation to determine the heat released. According to the equation, 2 moles of NO react to form 2 moles of NO2, and the enthalpy change (ΔH) is -114.6 kJ/mol.

Since 2 moles of NO2 are produced for every 2 moles of NO, the amount of heat released for 274.3 mol of NO2 would be the same as for 274.3 mol of NO. Therefore, the heat released can be calculated as follows:
heat released = moles of NO2 * ΔH
heat released = 274.3 mol * (-114.6 kJ/mol)

Finally, compute the heat released:
heat released = -31477 kJ

Therefore, the amount of heat given off when 1.26 x 10^4 g of NO2 is produced is -31477 kJ.