The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely.
2CO(g) + O2(g) --> 2CO2(g)
482 kJ x (12/2*28) = ?
Well, well, well! Looks like we've got quite the reaction going on here! Let's calculate the heat released, shall we?
First things first, we need to find the number of moles of CO(g) present in 12.0 g. To do this, we divide the mass by the molar mass.
The molar mass of CO is approximately 28 g/mol (12 g/mol for carbon and 16 g/mol for oxygen).
So, 12.0 g of CO(g) is equal to 12.0 g / 28 g/mol ≈ 0.4286 mol CO.
Hold onto your hat, because we're about to use the delta H value!
Since the reaction coefficient of CO is 2, it means that for every 2 moles of CO reacted, 2 moles of CO2 will be formed. So, for 0.4286 mol of CO reacted, we will get 0.4286 mol of CO2.
Now, we can calculate the heat released using the formula:
Heat released = moles of substance × delta H
Heat released = 0.4286 mol CO2 × (-482 kJ/mol)
Now, let's crunch the numbers:
Heat released ≈ -206.4 kJ
Oh dear, it seems like we've got ourselves a negative value! That means heat is being released to the surroundings. So, the heat released when 12.0 g of CO(g) reacts completely is approximately -206.4 kJ.
Stay cool, my friend!
To calculate the heat released to the surroundings when 12.0 g of CO (g) reacts completely, we need to use the concept of stoichiometry.
1. Convert the given mass of CO(g) to moles. To do this, we need to know the molar mass of CO, which is 28.01 g/mol.
Moles of CO = mass of CO / molar mass of CO
= 12.0 g / 28.01 g/mol
2. Determine the stoichiometric ratio between CO(g) and CO2(g) based on the balanced chemical equation.
From the balanced equation, we see that 2 moles of CO(g) produces 2 moles of CO2(g). Therefore, the stoichiometric ratio of CO(g) to CO2(g) is 1:1.
3. Use the stoichiometric ratio to calculate moles of CO2 produced.
Moles of CO2 = Moles of CO
4. Finally, calculate the heat released using the equation:
Heat released = moles of CO2 * dH
Heat released = Moles of CO * dH
Heat released = (12.0 g / 28.01 g/mol) * (-482 kJ)
Make sure to perform the calculations, and the resulting value will give you the heat released to the surroundings when 12.0 g of CO (g) reacts completely.
To calculate the heat released to the surroundings when 12.0 g of CO (g) reacts completely, we need to follow a few steps:
Step 1: Calculate the moles of CO(g)
To calculate the moles of CO(g), we use the molar mass of CO, which is 28.01 g/mol.
Moles of CO(g) = mass (g) / molar mass (g/mol)
Moles of CO(g) = 12.0 g / 28.01 g/mol ≈ 0.428 mol
Step 2: Use the balanced equation to determine the moles of CO₂ produced.
From the balanced equation, we can see that 2 moles of CO(g) react to produce 2 moles of CO₂(g).
Moles of CO₂(g) = moles of CO(g) / 2
Moles of CO₂(g) = 0.428 mol / 2 ≈ 0.214 mol
Step 3: Calculate the heat released using the given ΔH value
The given ΔH value is -482 kJ, which represents the heat released by 2 moles of CO₂(g). Therefore, we need to use a conversion factor to determine the heat released for 0.214 mol of CO₂(g).
Heat released (kJ) = moles of CO₂(g) x ΔH (kJ)
Heat released (kJ) = 0.214 mol x -482 kJ / 2 mol
Heat released (kJ) ≈ -51.4 kJ (rounded to one decimal place)
Therefore, the heat released to the surroundings when 12.0 g of CO(g) reacts completely is approximately -51.4 kJ.