Login or Sign Up
Menu
Ask a New Question

Determine the amount of heat (in kJ) given off when 1.26 Γ— 104𝑔 of NO 2 are produced according to the equation: 2𝑁𝑂(𝑔) + 𝑂2(𝑔) β†’ 2𝑁𝑂2(𝑔) βˆ†π» = βˆ’114.6π‘˜π‘—/π‘šπ‘œπ‘™

2𝑁𝑂(𝑔) + 𝑂2(𝑔) β†’ 2𝑁𝑂2(𝑔) βˆ†π» = βˆ’114.6π‘˜π‘—/π‘šπ‘œπ‘™

How many moles do you have in1.26 Γ— 104𝑔 (12,600 g) NO2?
So you get 114.6 kJ for 1 mol NO2 produced. You will get 2*114.6 kJ = 229.2 kJ for 2 mol NO2 produced. 2 mols NO2 = 2 mols x 46 g/mol = 92 grams; i.e., you will get 229.2 kJ for 92 g NO2 produced. How many kJ will you get for 12,600 g? That's
229.2 kJ x (12,600 g/92 g) = ? kJ.

Ah, heat production, the fiery topic! Well, to determine the amount of heat given off, we need to use the equation:

Δ𝐻 = -114.6 kJ/mol

Now, we have 1.26 Γ— 10^4 g of NO2, which we can convert to moles by dividing by the molar mass of NO2 (46.01 g/mol). So, let's crunch the numbers:

1.26 Γ— 10^4 g NO2 Γ— (1 mol NO2 / 46.01 g NO2) = 274.8 mol NO2

Since the stoichiometric coefficient of NO2 is 2 in the balanced equation, the heat produced in this case would be:

Δ𝐻 Γ— (2 mol NO2 / 1 mol) Γ— (274.8 mol NO2) = -114.6 kJ/mol Γ— 2 Γ— 274.8 mol = -62.9 kJ

So, it looks like approximately -62.9 kJ of heat would be given off. That's the "hot" gossip!

To determine the amount of heat given off when 1.26 Γ— 10^4 g of NO2 are produced, we need to use the equation βˆ†π» = βˆ’114.6 kJ/mol.

First, we need to find the number of moles of NO2 produced. To do this, we divide the given mass by the molar mass of NO2.

Molar mass of NO2 = (1 Γ— 14.01 g/mol) + (2 Γ— 16.00 g/mol)
= 46.01 g/mol

Number of moles of NO2 = (1.26 Γ— 10^4 g) / (46.01 g/mol)
β‰ˆ 273.81 mol

Next, we use the stoichiometry of the balanced equation to determine the amount of heat given off. From the balanced equation, we can see that for every 2 moles of NO2 produced, the reaction releases 114.6 kJ of heat.

βˆ†H per 2 moles of NO2 = -114.6 kJ

Now, we calculate the amount of heat given off for the number of moles of NO2 produced.

Amount of heat given off = (βˆ†H per 2 moles of NO2 / 2) Γ— Number of moles of NO2
= (-114.6 kJ / 2) Γ— 273.81 mol
β‰ˆ -6,573.51 kJ

Therefore, the amount of heat given off when 1.26 Γ— 10^4 g of NO2 are produced is approximately -6,573.51 kJ. Note that the negative sign indicates that heat is released in the reaction.

To determine the amount of heat (in kJ) given off when 1.26 Γ— 10^4 g of NO2 are produced, we can use the equation:

2NO(g) + O2(g) β†’ 2NO2(g)

where βˆ†H = -114.6 kJ/mol.

To solve this problem, we'll follow these steps:

1. Calculate the number of moles of NO2 produced.
2. Use the molar ratio between NO2 and βˆ†H to find the heat released.

Step 1: Calculate the number of moles of NO2 produced.
To find the number of moles, divide the given mass by the molar mass of NO2:

Molar mass of NO2 = (14.01 g/mol) + (2 * 16.00 g/mol) = 46.01 g/mol

Number of moles of NO2 = mass / molar mass
= (1.26 Γ— 10^4 g) / (46.01 g/mol)
β‰ˆ 273.86 mol

Step 2: Use the molar ratio between NO2 and βˆ†H to find the heat released.
According to the balanced equation, for every 2 moles of NO2, βˆ†H = -114.6 kJ.

Number of moles of NO2 with respect to βˆ†H = (273.86 mol / 2) β‰ˆ 136.93 mol

Heat released = βˆ†H * number of moles of NO2 with respect to βˆ†H
= (-114.6 kJ/mol) * (136.93 mol)
β‰ˆ -15,660.78 kJ

The amount of heat released when 1.26 Γ— 10^4 g of NO2 are produced is approximately -15,660.78 kJ. The negative sign indicates that the reaction is exothermic, meaning heat is given off.