54.0 g aluminum at 50.0oC is dumped into water at 38.5oC. The water warms to 40.0oC.

54.0 g aluminum at 50.0^oC is dumped into water at 38.5^oC. The water warms to 40.0^oC.

What is specific heat capacity of aluminum?

a) ____________

What is molar heat capacity of aluminum?

b) ____________

When 10.0 g ammonium nitrate is dissolved in 50.0 g water at 25.0^oC, the final temperature of the solution is 20.0^oC.

a. What is the q of the water? (SH water = 4.20 J/g K) (10 pt)

q_H2O _________

b. What is the molar change in enthalpy (ΔH in kJ/mol NH₄NO₃) for the solution process?

ΔH ___________

Solutions

Expert Solution

(1)

heat lost by Al = heat gained by water

mass of Al*SAl*DT = mass of water*S*DT

54*s*(50-40) = mass of water*4.184*(40-38.5)

mass of water not given

(2)

a) q of the water = m*s*DT

= (50)*4.2*(25-20)

= 1050 joule

qH2O = 1050 joule

b. no of mol of Al(NO3)3 dissolved = 10/213 = 0.047 mol

molar change in enthalpy (ΔH) = -q/n

= -1.05/0.047

DHrxn = -22.3 kj/mol

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of...

Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of water at 25.0°C. Determine the amount of steam (in g) needed for the system to reach a final temperature of 64.0°C. The specific heat of aluminum is 900 J/(kg · °C).

A 32.5 g cube of aluminum initially at 45.8C is submerged into 105.3 g of water...

A 32.5 g cube of aluminum initially at 45.8C is submerged into 105.3 g of water at 15.4C. What isthe final temperature of both substances at thermal equilibrium? (Assume that the aluminum and the water are thermally isolated) Please show all steps, not getting the algebra used to solve this.

A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g...

A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g piece of ice is cooled to −20.0 °C and then placed in the calorimeter. Use the following specific heats: cAl = 900.0 J Kg-1 °C-1, cwater = 4186 J Kg-1 °C-1, cice = 2.10 x 103 J Kg-1 °C-1. The latent heat of fusion for water is LF = 333.5 x 103 J/Kg. (a) Find the final temperature of the system, assuming no heat...

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water...

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water at 100 ∘C a) Determine the final temperature of the mixture. b) Determine the total change in entropy as a result of the mixing process (use ΔS=∫dQ/T).

aluminum sulfide and water react to form aluminum hydroxide and hydrogen sulfide gas. suppose 128.00 g...

aluminum sulfide and water react to form aluminum hydroxide and hydrogen sulfide gas. suppose 128.00 g of aluminum are added to 154.45 mL of water(d=1.00 g/ml). Answer the following questions. a).before the reaction, how many water molecules are present in the reaction mixture? b) when the reaction is finished. what mass, in g, of aluminum hydroxide can theoretically be produced? c) limiting reactant? d) mass in grams of remaining excessreactant if the theoretical yield of aluminum hydroxide is obtained? e)if...

15.00 g of aluminum sulfide (150.1 g/mol) and 10.00 g of water (18.02 g/mol) react until...

15.00 g of aluminum sulfide (150.1 g/mol) and 10.00 g of water (18.02 g/mol) react until the limiting reactant is used up. Calculate the mass of H2S (34.08 g/mol) that can be produced from these reactants. Notice that you will need to balance the reaction equation. ___Al2S3(s)+ ___H2O > ___Al(OH)3(s)+ ___H2S(g) 13.89 g d. 9.456 g 10.21 g e. 1.108 g 19.67 g

A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...

A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. A) Find the final temperature of the system, assuming no heat losses. (Assume that the specific heat of ice is 2.0 kJ/kg K) B) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? C) Would your answer...

A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...

A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. Find the final temperature of the system, assuming no heat losses. (Assume that the specific heat of ice is 2.0 kJ/kg K) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? Would your answer to part b...

The evaporation of water cools the surroundings, and the condensation of this vapor Does nothing Warms...

The evaporation of water cools the surroundings, and the condensation of this vapor Does nothing Warms the surroundings Increases the value of the latent heat of vaporization Decreases the value of the latent heat of vaporization The heat involved in the change of phase form solid ice to liquid water is Latent heat of vaporization Latent heat of fusion Latent heat of condensation None of the above More molecules are returning to the liquid state than are leaving the liquid...

18.7 g of aluminum and 226 g of chlorine gas react until all of the aluminum...

18.7 g of aluminum and 226 g of chlorine gas react until all of the aluminum metal has been converted to AlCl3. The balanced equation for the reaction is the following. 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) What is the quantity of chlorine gas left, in grams, after the reaction has occurred, assuming that the reaction goes to completion? (The formula mass of aluminum metal, Al, is 26.98 g/mol, and the formula mass of chlorine gas, Cl2, is...

Subjects