If 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius, how much water at 0 degrees Celsius is produced? How much ice is left? The molar heat of melting is 6.01 kJ/mol.
So... 6.01 kJ -> 1 mol (6.01 kJ of energy can melt 1 mole of ice)
Then... 13.4 kJ -> x (How many moles of ice are melted by 13.4 kJ of energy?)
x = 2.23 mol (2.23 mol of ice melted by 13.4 kJ of energy)
What's next?
Yes, 2.23 mols ice are melted? How many grms is that? grams = mols x molar mass = approx 40 g. How much ice did you have? That's 1,000 g. How much ice is left. Approx 1000-40 = ?
Question text
Calculate the energy required to melt 21 g of ice at 0 oC.
The molar heat of fusion for ice is 6.02 kJ/mol.
Answer kJ
Next, we need to calculate the amount of water produced.
Since each mole of ice (H2O) is equivalent to one mole of water (H2O), we can say that 2.23 mol of ice will produce 2.23 mol of water.
To convert moles of water to mass, we need to use the molar mass of water, which is 18.015 g/mol.
Thus, the mass of water produced can be calculated as follows:
2.23 mol * 18.015 g/mol = 39.98 g of water
Therefore, 39.98 grams of water at 0 degrees Celsius is produced when 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius.
Now, let's calculate the amount of ice left.
The initial mass of ice was 1.00 kg, which is equivalent to 1000 g.
The mass of water produced was 39.98 g.
Therefore, the amount of ice left can be calculated as follows:
Initial mass of ice - Mass of water produced
= 1000 g - 39.98 g
= 960.02 g
Thus, there will be 960.02 grams of ice left after 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius.
Next, we need to determine the amount of ice that corresponds to 2.23 moles. We can use the molar mass of water to convert moles of ice to grams of ice.
The molar mass of water (H2O) is approximately 18.015 grams/mole. Therefore, to convert moles to grams, we can use the following conversion factor:
1 mole H2O = 18.015 grams H2O
Now we can calculate the mass of ice that corresponds to 2.23 moles:
2.23 mol H2O × 18.015 g H2O/mol = 40.12 g of ice
Therefore, 2.23 moles of ice is equal to approximately 40.12 grams of ice.
Since 1 kilogram of ice was initially present, we can subtract the mass of ice that melted (40.12 g) from the initial mass of ice (1000 g) to find the mass of ice that is left:
1000 g - 40.12 g = 959.88 g of ice
So, approximately 959.88 grams of ice are left after 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius.
To determine the amount of water produced, we need to consider that the initial mass of ice has been reduced by the mass of ice that melted (40.12 g). Therefore, the mass of water produced is:
1000 g - 40.12 g = 959.88 g
So, approximately 959.88 grams of water at 0 degrees Celsius are produced.