Question

In: Chemistry

How much heat, in kJ, is absorbed by a 77.0 g sample of aluminum at 25.0°C...

How much heat, in kJ, is absorbed by a 77.0 g sample of aluminum at 25.0°C when it is immersed in boiling water? The specific heat capacity of aluminum is 0.900 J/g°C and the specific heat capacity of water is 4.184 J/g°C. Enter your answer with no units.

Need some help on this one. Please show work/relevant formulas. Thanks for any help!

Solutions

Expert Solution

Heat absorbed by aluminium, Q = mcdt

Where

m = mass of aluminium = 77.0 g

c = specific heat capacity of aluminum = 0.900 J/g°C

dt = change in temperature of aluminium = final temperature - initial temperature

    = 100 - 25

   = 75 oC

Plug the values we get Q = mcdt

                                     = 77.0x0.900x75 J

                                    = 5.2 x103 J

                                    = 5.2 kJ                Since 1kJ = 103 J

Therefore the heat absorbed is 5.2 kJ


Related Solutions

How much energy (kJ) is required to convert a 25.0 g ice cube at -15.°C to...
How much energy (kJ) is required to convert a 25.0 g ice cube at -15.°C to water vapor at 250°C?
how much heat (in kj) is needed to convert 866 g of ice at -10 c...
how much heat (in kj) is needed to convert 866 g of ice at -10 c to steam at 126 c? spH of ice and steam are 2.03J/g*c and 1.99J/g*c, respectively.
How much heat (in kJ) is needed to convert 866 g of ice at −10.0°C to...
How much heat (in kJ) is needed to convert 866 g of ice at −10.0°C to steam at 126.0°C? (The specific heats of ice, water, and steam are 2.03 J/g · °C, 4.184 J/g · °C, and 1.99 J/g · °C, respectively. The heat of fusion of water is 6.01 kJ/mol, the heat of vaporization is 40.79 kJ/mol.)
How much heat in kilojoules is evolved or absorbed in the reaction of 292.5 g of...
How much heat in kilojoules is evolved or absorbed in the reaction of 292.5 g of calcium oxide with enough carbon to produce calcium carbide? CaO(s)+3C(s)→CaC2(s)+CO(g) ΔH∘ = 464.6kJ
How much heat (in kJ) is required to convert 423 g of liquid H2O at 25.2°C...
How much heat (in kJ) is required to convert 423 g of liquid H2O at 25.2°C into steam at 156°C? (Assume that the specific heat of liquid water is 4.184 J/g·°C, the specific heat of steam is 2.078 J/g·°C, and that both values are constant over the given temperature ranges. The normal boiling point of H2O is 100.0°C.)
A sample of 58.90 g solid benzene at −2.3°C was heated until it absorbed 13.2 kJ...
A sample of 58.90 g solid benzene at −2.3°C was heated until it absorbed 13.2 kJ of heat, at a constant pressure of 1 atmosphere. Using the data given in the table below, determine the final phase and final temperature of the benzene sample. Properties of Benzene Values melting point 5.49°C boiling point 80.09°C heat of fusion at 5.49°C 9.87 kJ/mol heat of vaporization at 80.09°C 30.72 kJ/mol molar heat capacity of solid at 0°C 118.4 J/mol·K molar heat capacity...
when 1.0 mol of NO(g) forms from its elements, 90.29 kJ of heat is absorbed. How...
when 1.0 mol of NO(g) forms from its elements, 90.29 kJ of heat is absorbed. How much heat is evolved when 5.40 g of NO decomposes to its elements?
How much heat (in kJ) is required to warm 13.0 g of ice, initially at -15.0...
How much heat (in kJ) is required to warm 13.0 g of ice, initially at -15.0 ∘C, to steam at 110.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C.
How much heat (in kJ) is required to warm 11.0 g of ice, initially at -11.0...
How much heat (in kJ) is required to warm 11.0 g of ice, initially at -11.0 ∘C, to steam at 114.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C.
How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0...
How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0 ∘C, to steam at 114.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C, the heat of fusion for water is 6.02 kJ/mol, and the heat of vaporization for water is 40.7 kJ/mol.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT