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- 35dm3 of hydrogen is produced at a total pressure of 1 atm by the action of acid on a metal. Calculate the workdone by the gas in pushing back the atm in a. dm3 atm b. joules.At constant pressure and 25^C, What is delta H for the following reaction. 2C2H6(g) + 7O2(g) = 4CO2(g) + H2O(l) if the complete consumption of 38.2 g of C2H6 libraties 1981 KJ of heat energy?How do I state the conditions of spontaneity on problem 7?
- Calculate the amount of energy released as heat by the formation of 1.00 mL of water from a stoichiometric mixture of H2(g) and O2(g) at 25°C and a constant pressure of one bar. Calculate the amount of energy released as heat by this reaction per mole and per gram of H2(g). Take the density of water to be 1.00 grams per milliliter. Answers: −15.9 kJ; −286 kJ·mol–1; −142 kJ·g–1Natural gas is very abundant in many Middle Eastern oilfields. However, the costs of shipping the gas to markets inother parts of the world are high because it is necessary toliquefy the gas, which is mainly methane and has a boilingpoint at atmospheric pressure of -164 °C. One possiblestrategy is to oxidize the methane to methanol, CH3OH,which has a boiling point of 65 °C and can therefore beshipped more readily. Suppose that 10.7 * 109 ft3 of methaneat atmospheric pressure and 25 °C is oxidized to methanol.(a) What volume of methanol is formed if the densityof CH3OH is 0.791 g>mL? (b) Write balanced chemicalequations for the oxidations of methane and methanol toCO21g2 and H2O1l2. Calculate the total enthalpy changefor complete combustion of the 10.7 * 109 ft3 of methanejust described and for complete combustion of the equivalentamount of methanol, as calculated in part (a).(c) Methane, when liquefied, has a density of 0.466 g>mL;the density of methanol at 25 °C is 0.791…What would be the equilibrium temperature if you drop 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) into 105 g of water (Cp = 4.184 J/g-oC,initially at 23oC)?
- Suppose that H2O (l) goes from 29.0oC and 1 atm to 31.0oC and pressure P2. What value of P2 would make ∆S=0 for this process?How much energy (at constant temperature and pressure) must be supplied as heat to 10.0 g of chlorine gas (as Cl2) to produce a plasma composed of Cl- and Cl+ ions? The enthalpy of ionization of Cl(g) is +12575 kJ mol-1 and its electron gain enthalpy is -349 kJ mol-1. Hence identify the standardenthalpy of ionization of Cl- (g).Oxyacetylene torches rely on a precise mixture of fuel (C2H2(g)) to oxygen to optimize the welding process. _ C2H2 (g) + _ O2 (g) ---> CO2 (g) + _H2O (g) Calculate the volume (in L) of O2(g) required to react completely with 14.5 L of acetylene. Assume both substances are at SATP.