24.1 kJ of energy is lost by a 251 g Al block. If the block is initially at 125.0°C what will be its final T in °C? (sAl = 0.902 J g-1 °C-1)
0.55 g of isopropyl alcohol (C3H8O) evaporates from a 36.31 g aluminum block initially at 25.0 °C. Calculate the final temperature of the aluminum block. Assume 100% heat transfer. Isopropyl alcohol: at its boiling point ΔHvap = 39.9 kJ/mol; at 25 °C ΔHvap = 45.4 kJ/mol. Heat capacity of Al(s) = 0.903 J/(g °C). answer is 12.3, show work
Please help solve and show work. Review Constants 1 Pe A 27.5-g aluminum block is warmed to 65.0 °C and plunged into an insulated beaker containing 55.0 g of water initially at 22.2°C. The aluminum and the water are allowed to come to thermal equilibrium. ( Cs,H20 = 4.18 J/g • °C, Cs, al = 0.903 J/g • °C) Part A Assuming that no heat is lost, what is the final temperature of the water and aluminum? IVO ALQ R...
please show work 19. A 35.0 g block of copper is put into 125.0 g of water to cool. The copper block cools down from 75.0 c to 25.0°c. What was the change in energy for the copper in this process? 16 points) 20. Using Hess's law, calculate the enthalpy of formation for the following reaction: CHIg) + 201g)-> CO,(g) + 2H20(g) ΔΗ ? c(s) + 2H2(g) .> CH4 (g) c(s) + Odg) .> CO2(g) Hz(g) + 02 (g)-> H2O...
When H2(g) reacts with O2(g) according to the following reaction, 242 kJ of energy are evolved for each mole of H2(g) that reacts. Complete the following thermochemical equation. 2H2(g) + O2(g)— 2H2O(g) AH- The following information is given for bismuth at latm: T = 1627.00°C T. = 271.00°C Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C AHvap (1627.00°C) = 822.9 J/g AH (271.00°C) = 52.60 Jig A 38.40 g sample of liquid bismuth at...
3. A 100 g block of copper initially at 60°C is placed in contact with a 300 g block of aluminum initially at 30°C in an insulated container. A. Identify the block that loses thermal energy. (5 pts) B. Calculate the final equilibrium temperature of the two blocks. (15 pts) Copper a(Cu) = 17 x 10-61°C Ccu = 0.0923 cal/g.K = 386 J/kg-K LF (Cu) = 207 kJ/kg
The gas in a piston (defined as the system) is warmed and absorbs 655 J of heat. The expansion performs 348 J of work on the surroundings. Part A What is the change in internal energy for the system? ΔE = J A system releases 617 kJ of heat and does 145 kJ of work on the surroundings. Part A What is the change in internal energy of the system? ΔE = kJ A 31.2 g wafer of pure gold...
2 2.50 kj of heat energy is applied to 25.0 g piece of aluminum at 25.0 degrees C. pt Given that the specific heat capacity of Al is 0.878 J/gC, what is the final temperature of the metal? 138.9 degrees C 134.1 degrees C 113.9 degrees C 88.9 degrees C
A 150.0 g block of iron absorbs 750.0 J of thermal energy. The specific heat capacity of iron is 0.449 J/(g·◦C). The initial temperature of the block is 20.0 ◦C. What is its final temperature? (A) 111.3 ◦C (B) 31.1 ◦C (C) 22.2 ◦C (D) 20.4 ◦C (E) 8.86 ◦C
Three separate 3.50 g blocks of Al, Cu, and Fe at 25.0C each absorb 0.505 kJ of heat. Which block shows the highest change in temperature and what is this change in temperature? The specific heats of Al, Cu, and Fe are 0.900 J/g·K, 0.385J/g·K, and 0.444 J/g·K, respectively.
After transfer of 1.60 kJ of thermal energy to a 0.451-kg block of copper the temperature is 44.1 °C. The specific heat capacity of copper is 0.385 J g-1 °C-1. Calculate the initial temperature of the copper.