what is the energy needed to melt 5.62 moes of ice in 0'C
To calculate the energy needed to melt a certain amount of ice, you can use the equation:
Q = m * ΔHf
Where:
Q = energy needed (in joules)
m = mass of ice (in moles)
ΔHf = heat of fusion (in joules per mole)
To find the heat of fusion, we need to know the specific heat of fusion for water, which is 334000 J/mol.
First, convert the moles of ice to grams using the molar mass of water (18 g/mol):
5.62 moles * 18 g/mol = 101.16 grams
Next, plug the values into the equation:
Q = 101.16 g * 334000 J/mol
Calculate the energy needed:
Q = 33815840 J
Therefore, the energy needed to melt 5.62 moles of ice at 0°C is approximately 33,815,840 joules.
To calculate the energy needed to melt a certain amount of ice, you need to use the equation:
Q = m * ΔH
where:
Q is the energy needed (in Joules),
m is the mass of the ice (in moles),
ΔH is the enthalpy of fusion (heat of fusion) of ice, which is 6.02 kJ/mol.
First, you need to convert the mass of the ice from moles to grams. The molar mass of water is approximately 18 g/mol.
mass of ice (in grams) = moles of ice * molar mass of water
mass of ice (in grams) = 5.62 moles * 18 g/mol
Next, you can calculate the energy needed using the equation above:
Q = mass of ice * ΔH
Q = (5.62 moles * 18 g/mol) * (6.02 kJ/mol * 1000 J/kJ)
Simplifying this equation gives you the value of Q, which is the energy needed to melt the given amount of ice at 0°C.