Calculate the energy change when 50.0 g of ice melts (H fusion = 334 kJ/mol). Molar mass for water 18 g/mol
in simple steps
To calculate the energy change when 50.0 g of ice melts, we can use the equation:
Energy Change = Mass of Substance x Heat of Fusion.
1. Convert the mass of ice from grams to mols:
50.0 g / 18 g/mol = 2.77 mol
2. Calculate the energy change using the heat of fusion:
Energy Change = 2.77 mol x 334 kJ/mol = 925.18 kJ
Therefore, the energy change when 50.0 g of ice melts is 925.18 kJ.
To calculate the energy change when ice melts, we can use the following steps:
Step 1: Calculate the number of moles of ice:
Given mass of ice = 50.0 g
Molar mass of water (H2O) = 18 g/mol
Number of moles of ice = (mass of ice) / (molar mass of water)
= 50.0 g / 18 g/mol
= 2.78 mol (approx.)
Step 2: Calculate the energy change using the given enthalpy of fusion:
Given enthalpy of fusion (H fusion) = 334 kJ/mol
Energy change = (number of moles) x (enthalpy of fusion)
= 2.78 mol x 334 kJ/mol
= 928.52 kJ (approx.)
Therefore, the energy change when 50.0 g of ice melts is approximately 928.52 kJ.
To calculate the energy change when 50.0 g of ice melts, we need to use the equation:
Energy change = (Mass of ice / Molar mass of water) * Heat of fusion
Now, let's break down the calculation into simple steps:
Step 1: Convert the mass of ice to moles.
Molar mass of water = 18 g/mol
Mass of ice = 50.0 g
To find the number of moles, divide the mass of ice by its molar mass:
Number of moles = Mass of ice / Molar mass of water
Number of moles = 50.0 g / 18 g/mol
Step 2: Calculate the energy change using the equation:
Energy change = (Number of moles) * Heat of fusion
The heat of fusion is given as 334 kJ/mol.
Energy change = (Number of moles) * Heat of fusion
Energy change = (50.0 g / 18 g/mol) * 334 kJ/mol
Step 3: Calculate the final result.
Multiply the number of moles by the heat of fusion to get the energy change.
Final Result:
Energy change = (50.0 g / 18 g/mol) * 334 kJ/mol