How much heat energy is required to convert 35.8 g of liquid sulfur dioxide, SO2, at 207.5 K to gaseous SO2 at 263.1K if the molar heat of vaporization of SO2 is 24.9 kJ/mol, and the specific heat capacity (?) of liquid SO2 is 1.36 J/(g·∘C)? Give q in kj.

88.0 g copper at the temperature of 77.00  oC is dropped into 100. g water at 25.00 o C.   If the exchanged  heat   is used to melt 10.0 g of solid sample.  Calculate  the  heat of fusion for the solid in kJ/ mole. The mailer mass of solid is 71.0 g/ mole.  CP of H2O (l) = 4.84 J / g oC CP of Cu (s) = 0.385 J / g oC.

How much heat energy is required to convert 74.9 g of solid iron at 27⁢ ∘C to liquid iron at 1538⁢ ∘C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538⁢ ∘C. The specific heat capacity of solid iron is 0.449 J/(g·∘C). q=       kj

Calculate the heat absorbed when 35.39 g of some substance at 13.16°C is completely melted. The molar heat of fusion for the substacnce is 5.91kJ · mol, and the molar mass is 16.45g · mol Exproco

A compound has a vapor pressure of 100 mmHg at 267 K and a normal boiling point of 338 K.  What is the ΔHvap for this compound in kJ/mol?

Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro

(a) Consider a substance where the intermolecular forces hold the molecules in fixed rigid positions. What is the process called when enough heat has been added to the substance so that the molecules begin to flow? (b) Consider a substance where the intermolecular forces hold the molecules in close contact with each other, but the molecules can flow. What is the process called when enough heat has been added to the substance so that the molecules escape each other? (c) Consider a substance where the intermolecular forces hold the molecules in fixed rigid positions. What is the process called when enough heat has been added to the substance so that the molecules can escape each other?

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The amount of heat produced in an "ice calorimeter " is determined from the quantity of ice that melts, knowing that it takes 7.01 kJ of heat to melt exactly 1 mol of ice. Suppose that a 1.45-g sample of Al2O3(s) at 60.6 °C is dropped into an ice calorimeter. How many grams of ice will melt?

With around 70% of ammonia produced industrially being used to make fertilizers. The specific heat capacity of liquid ammonia is 80.8 J/g*K while that of gaseous ammonia is 37.0 J/g*K. Given that the boiling point and enthalpy of vaporization of ammonia is -33.3°C and 23.5 kJ/mol, respectively, how much energy is required to heat 75 g of ammonia (17.03 g/mol) from the temperature of liquid nitrogen (-195.8°C) to room temperature (25.0°C)?