How much heat is required to melt 56.0 g of ice at its melting point?
Latent heat of fusion of ice = 333.6 J/g
Mass = 56.0 g
Use:
Q = Lf*mass
= (333.6 J/g)*56.0 g
= 1.87*10^4 J
Answer: 1.87*10^4 J
How much heat is required to melt 56.0 g of ice at its melting point?
1. How much heat is required at constant pressure to melt 1 mole of ice at -25 C to steam at 125° C? boiling point 100c melting point 0.000'C specific heat capacities are gas(steam) 2.08, liquid 4.184 solid (ice) 2.11. All in units of JigC AH(100°C) 40.7 kJ/mol AHu (0.000°C)-6.01 kJ/mol 2. Calculate AHrxn for the reaction: CH4(g)4 Cl2(g) -CC4(g) 4 HCl (g) + Use the following reactions and given AH's: CH4(g) AH =-74.6 kJ 2 H2(g) C(s) C(s)2 Cl2(g)...
calculate the heat required to melt 9.73 g of benzene at it's normal melting point nd Phases (References] a. Calculate the heat required to melt 9.73 g of benzene at its normal melting point. Heat of fusion (benzene) 9.92 kJ/mol Heat = kJ b. Calculate the heat required to vaporize 9.73 g of benzene at its normal boiling point. Heat of vaporization (benzene) = 30.7 kJ/mol Heat = kJ Submit Answer Try Another Version 2 item attempts remaining arch о...
How much heat does it take to melt 43.77 g of copper if the copper is already at its melting point? The heat of fusion of copper is 49cal/g
At 1 atm, how much energy is required to heat 0.0550 kg of ice at -22.0 °C to steam at 129.0 °C? STRATEGY 1. Calculate the energy needed for each temperature change or phase change individually. A. The energy needed to heat 0.0550 kg of ice from -22.0 C to its melting point. B. The energy needed to melt 0.0550 kg of ice at its melting point C. The energy needed to heat 0.0550 kg of liquid water from the...
How much heat is required to melt 4.30 kg of ice with an initial temperature of 0 degC, and turn it into steam at 100 degC?
The enthalpy of fusion for methane (CH4) is 0.942kJ/mol. How much heat is required to melt 37.91g of solid methane at its melting point? Report your answer in units of kJ.
What quantity of heat would be needed to melt 1.00 g rubidium at its normal melting point? Heat = J What quantity of heat would be needed to vaporize 1.00 g rubidium at its normal boiling point? Heat = J What quantity of heat would be evolved if 1.00 g rubidium vapor condensed at its normal boiling point?
3. How much energy (in kJ) is required to get a 100. g ice cube at -10.0°C to completely melt? (HINT: Which AH andispecific heat (e) are used for melting solid to a liquid?)
how much heat is needed to melt 30g of ice at 0c qfus = 80cal/g cal/g=334
How many kilocalories are required to melt 503 g of ice at 0°C. Latent heat of fusion for ice is 80 cal/g. 6