i think I'm using the wrong formula
i think I'm using the wrong formula must be added to 126.00 g of ice at...
A total of 619 cal of heat is added to 5.00 g of ice at −20.0 °C. What is the final temperature of the water? Specific heat of ?2?(?) 2.087 J/(g⋅°C) Specific heat of ?2?(?) 4.184 J/(g⋅°C) Heat of fusion for ?2? 333.6 J/g
6) There is 15.0 g of ice at 0.0C. How many grams of water at 50.0C must be added to the ice to melt all the ice and keep the temperature of the mixture at 0.OC? H2O(s)= 2.06J/gc Specific heat: H2O(0) = (4.18 J/g C) H20 heat of vaporization=2260 J/g H2O(g)=(2.03 J/g C) H2O heat of fusion=333 J/g b)25 8 c)23.98 d)7. 58 )0.428
An ice cube with a mass of 46.4 g at 0.0 ∘C is added to a glass containing 4.20×102 g of water at 45.0 ∘C . Determine the final temperature of the system at equilibrium. The specific heat capacity of water, ?s , is 4.184 J/g⋅∘C , and the standard enthalpy of fusion, Δ?∘fus , of water is 6.01×103 J/mol . Assume that no energy is transferred to or from the surroundings.
An ice cube with a mass of 53.0 g at 0.0 °C is added to a glass containing 368 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs, is 4.184 J/g·°C and the standard enthalpy of fusion, ΔH°fus, of water is 6.01 × 103 J/mol. Assume that no energy is transferred to or from the surroundings.
An ice cube of mass 9.0g is added to a cup of coffee, whose temperature is 90.0 °C and which contains 120.0 g of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0kJ/mol. Find the temperature of the coffee after the ice melts. Use the equation given in the lab manual on page 86. Ignore the + (CC) (AT)...
Given 464.0 g of hot tea at 76.5 ∘C, what mass of ice at 0 ∘C must be added to obtain iced tea at 11.0 ∘C? The specific heat of the tea is 4.18 J/(g⋅∘C), and ΔHfusion for ice is +6.01 kJ/mol.