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The specific heat of gold is 0.129 J/g°C. What is the molar heat capacity of gold?...
TC01E13 Calculate 9 (heat) for a system consisting of 29.5 g of gold (Cp = 0.129 J/K/g) when its temperature was raised from 26.2 °C to 94.7 °C. Select one: O a. 261 J O b. 261 kJ/mol C. 15665 J d. 1300 J e. 1300 J/mol
TC01E13 Calculate 9 (heat) for a system consisting of 29.5 g of gold (Cp = 0.129 J/K/g) when its temperature was raised from 26.2 °C to 94.7 °C. Select one O a. 261 J O b. 261 kJ/mol o C. 15665 J O d. 1300 J o e. 1300 J/mol
The specific heat capacity of silver is 0.24 J/°C .g. (a) Calculate the energy required to raise the temperature of 140.0 g Ag from 273 K to 305 K. (b) Calculate the energy required to raise the temperature of 1.0 mol Ag by 1.0°C (called the molar heat capacity of silver). O J/mol°C (c) It takes 1.35 kJ of energy to heat a sample of pure silver from 12.0°C to 15.3°C. Calculate the mass of the sample of silver. 9
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
. A 6.75 g sample of gold (specific heat capacity = 0.130 J/g。C) is heated using 50.6 J of energy. If the original temperature of the gold is 25.0°C, what is its final temperature? A. 24.4°C C. 82.7°C D. 43.4°C
If 400 J of heat were added to 100 g copper (specific heat = 0.385 J/g°C) and 400 J were added to 100 g of gold (specific heat = 0.129 J/g°C), which metal, copper or gold, would have the lower final temperature?
If the specific heat capacity of a metal is 0.352 J/g*C - what is the approximate molar mass of the metal?
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
water has a molar heat capacity of 75.38 J/(mol 12. Water has a molar heat capacity of 75.38 J/(mol x °C) and its vaporization enthalpy at 100°C is 40.7 kJ/mol. How much energy is needed to convert 36 g liquid H20 at 70.0°C to steam at 100°C? A) 85.9 kJ B) 126 kJ C) 77.6 kJ D) 81.4 kJ E) 45.2 kJ
The molar heat capacity of a compound with the formula C2H6SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.