Calculate the amount of heat required to completely sublime 76.0g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.

Would you believe

q = 76.0g x (1 mol/44g) x 32.3 kJ/mol = ?

55.8

Well, isn't dry ice just the coolest thing? See what I did there? Anyway, let's crunch some numbers!

First, we need to convert the mass of dry ice from grams to moles. The molar mass of CO2 is about 44 g/mol, so 76.0g of dry ice is approximately 76.0g / 44 g/mol ≈ 1.73 mol.

Now, we multiply the number of moles by the heat of sublimation. 1.73 mol * 32.3 kJ/mol = 55.899 kJ.

So, the amount of heat required to completely sublime 76.0g of dry ice is approximately 55.899 kJ.

That's a lot of heat! It's almost as if dry ice just vanished into thin air. Poof! 😄

To calculate the amount of heat required to completely sublime 76.0g of solid dry ice (CO2) at its sublimation temperature, we need to first convert the mass of CO2 from grams to moles. Then we can use the molar heat of sublimation to find the total heat.

Step 1: Convert grams to moles
To convert grams to moles, we need the molar mass of CO2, which is 44.01 g/mol.

76.0g CO2 × (1 mol CO2 / 44.01 g CO2) = 1.727 mol CO2

Step 2: Calculate the heat required
The molar heat of sublimation for carbon dioxide is given as 32.3 kJ/mol.

Heat required = 1.727 mol CO2 × 32.3 kJ/mol = 55.8271 kJ

Therefore, the amount of heat required to completely sublime 76.0g of solid dry ice at its sublimation temperature is approximately 55.83 kJ.

To calculate the amount of heat required to sublime solid dry ice (CO2), you need to use the equation:

q = m * ΔHsub

Where:
q = amount of heat (in joules)
m = mass (in grams)
ΔHsub = heat of sublimation (in joules/gram)

First, convert the mass of the solid dry ice from grams to moles. To do this, you need to know the molar mass of carbon dioxide (CO2).

The molar mass of CO2 is:
12.01 g/mol (C) + 2 * 16.00 g/mol (O) = 44.01 g/mol

Next, calculate the number of moles of CO2 in 76.0 g by dividing the mass by the molar mass:

76.0 g CO2 * (1 mol CO2 / 44.01 g CO2) = 1.73 mol CO2

Now that you have the number of moles of CO2, you can calculate the amount of heat required to sublime the solid dry ice by using the equation:

q = m * ΔHsub

q = 1.73 mol CO2 * (32.3 kJ/mol) * (1000 J/1 kJ)

Convert kJ to J to have consistent units:

q = 1.73 mol CO2 * (32.3 kJ/mol) * (1000 J/1 kJ)
= 55,879 J

Therefore, the amount of heat required to completely sublime 76.0 g of solid dry ice at its sublimation temperature is 55,879 Joules.