Question

In: Chemistry

A 31.87 g sample of a substance is initially at 28.5 °C. After absorbing 1697 J...

A 31.87 g sample of a substance is initially at 28.5 °C. After absorbing 1697 J of heat, the temperature of the substance is 140.5 °C. What is the specific heat (c) of the substance?

Solutions

Expert Solution

Given, mass of sample (m)= 31.87 gm

           Initial temperature (T1) = 28.50C

           Final temperature (T2) = 140.50C

          Hence, T = T2 - T1 = 140.50C - 28.50C = 1120C

          Heat absorbed (q) = 1697 J

          Specific heat (C) = ???

As we know,

               q = m*C*T

              C = q / m*T

              C = 1697 J / 31.87 gm * 1120C

              C = 1697 J / 3569.44 gm0C

              C = 0.475 J/gm0C


Related Solutions

1)A 55.67 g sample of a substance is initially at 22.7 °C. After absorbing 2847 J...
1)A 55.67 g sample of a substance is initially at 22.7 °C. After absorbing 2847 J of heat, the temperature of the substance is 132.2 °C. What is the specific heat (c) of the substance? 2)An 80.0-gram sample of a gas was heated from 25 °C to 225 °C. During this process, 346 J of work was done by the system and its internal energy increased by 7785 J. What is the specific heat of the gas? 3)How much work...
An unknown mass of each substance, initially at 25.0 ∘C, absorbs 1930 J of heat. The...
An unknown mass of each substance, initially at 25.0 ∘C, absorbs 1930 J of heat. The final temperature is recorded. Find the mass of each substance. a. Pyrex glass (Tf= 55.6 ∘C) sand (Tf= 62.1 ∘C) ethanol (Tf= 44.3 ∘C) water (Tf= 32.3 ∘C)
A 49.5 g sample of a substance which contains C, H, and O is burned in...
A 49.5 g sample of a substance which contains C, H, and O is burned in excess oxygen, producing 110.0 g of CO2 and 22.5 g of H2O. A mass spectrum confirms that the molar mass of the sample is 162.0 g/mol. a.) how many moles and grams of carbon were in the original sample? b.) How many moles and grams of hydrogen were in the original sample? c.) How many moles and grams of oxygen were in the original...
A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a...
A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a 10.00 g sample of iron (specific heat capacity = 0.45 J °C-1 g-1) are heated to 100.0 °C. The mixture of hot iron and aluminum is then dropped into 91.9 g of water at 23.7 °C. i) State the conditions for phase equilibrium of this system. NOTE: For an isolated system, the equilibrium state corresponds to the state with maximum entropy.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
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 20.4 g of steam at 162°C is condensed, cooled, and frozen to ice at -50.°C.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
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 13.2 g of steam at 192°C is condensed, cooled, and frozen to ice at -50.°C.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
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 27.1 g of steam at 216°C is condensed, cooled, and frozen to ice at -50.°C. ______KJ Please show the steps
10.0 g of a substance at 60.0°C is placed into 20.0 g water at 5.00°C. The...
10.0 g of a substance at 60.0°C is placed into 20.0 g water at 5.00°C. The final temperature of both materials is 12.0°C. What is the specific heat of the unknown material?
An 65.73 g sample of aluminum is placed on a 56.35 g sample of copper initially...
An 65.73 g sample of aluminum is placed on a 56.35 g sample of copper initially at 111.86oC. If the heat is only transferred between the metals (with no loss to the surroundings) and the final temperature of both metals is 36.38oC, what is the inital temperature (in oC) of aluminum?
Specific heat of ice: 2.09 J/(g⋅∘C Specific heat of liquid water: 4.18 J/(g⋅∘C) Enthalpy of fusion:...
Specific heat of ice: 2.09 J/(g⋅∘C Specific heat of liquid water: 4.18 J/(g⋅∘C) Enthalpy of fusion: ΔHfus=334J Enthalpy of vaporization: ΔHvap=2250 J/g How much heat energy, in kilojoules, is required to convert 47.0 g of ice at −−18.0 ∘C∘C to water at 25.0 ∘C?
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT