Consider the reaction of aluminum metal with hydrochloric acid. 2 Al(s) + 6 HCl(aq) →2 AlCl3(aq) + 3 H₂(g) When 5.00 g of aluminum is added to an excess of hydrochloric acid, all at a constant pressure of 1 atm and a constant temperature of 298 K, the system expels 99.8 kJ of heat into the surroundings. Calculate the number of moles of hydrogen gas that are produced. Assume that the heat is exchanged without a change in temperature. calculate the amount of work done by the systen when the hydrogen gas expands against a constant-pressure atmosphere of 1 atm at 298 K. (Use R = 8.314 x 10³ kJ mol-¹ K-¹.) Use the sign conventions of heat and work and the First Law of Thermodynamics calculate the change in internal energy of the system.

The reaction of carbon monoxide(g) with water(l) to form carbon dioxide(g) and hydrogen(g) proceeds as follows: CO(g) + H2O(l)  ---> CO2(g) + H2(g) When 10.2 grams of CO(g) react with sufficient H2O(l) , 1.02 kJ of energy are absorbed .What is the value of H for the chemical equation given?

(d) Determine the weight percentage, wt%, of the solid solution and liquid solution of a Cu-Ni alloy with a composition of 21 % Ni 79 % Cu, at a temperature of 1050 °C. Use part of the Thermal Equilibrium Diagram for Copper (Cu)-Nickel (Ni) alloy, as shown in Figure 1. Clearly show all your calculations. Temperature "C Figure 1 Part of the Cu-Ni thermal equilibrium diagram (not to scale) 1050 11 21 29 % Ni

The fuel in the form of biogas (65%-mol CH4 and 35%-mol CO2) is burned in a furnace. In order for combustion to take place stoichiometrically, calculate the air to fuel ratio (vol/vol) from this problem!

Question: Consider the sugar–water phase diagram of Figure 10.1.                (a)  How much sugar will dissolve in 1000 g of water at 80°C (176°F)?                (b)  If the saturated liquid solution in part (a) is cooled to 20°C (68°F), some of the sugar will precipitate out as a solid.  What will be the composition of the saturated liquid solution (in wt% sugar) at 20°C?                (c)  How much of the solid sugar will come out of the solution upon cooling to 20°C?   Figure 10.1 is provided below.

4. At 1084 °C solid copper melts to form a liquid. The phase change can be described as Cu(s) → Cu(t). The density of solid and liquid copper are 8.96 g/cm' and 7.75 g/cm' respectively. The enthalpies of combustion of the solid and liquid are -156.06 kJ/mol and -167.92 kJ/mol respectively. The product of combustion of both the solid and liquid is CuO(s). Calculate the standard enthalpy changes for the fusion process in kJ/mol. Calculate the change in internal energy when the sample is under a pressure of 500 kbar. Cu(s) → Cu(e) Solid copper liquid copper enthalples of combustion 8.96 g/cm3 7.75 g 1cm² said: -156.06 kJ/mol liquid-162.42 kJ/mol