4. Use the information below to calculate Sº 3 PbBr2(s) Pb²+ (aq) + 2 Br(aq) Substance AHºf (kJ/mol) so (J/K) Pb2+ (aq) -1.7 10.5 Br (aq) -121.5 82.4 PbBr2(s) -282.4 ??? Report your answer in J/K with one decimal place, but do not write the units. Include a for BaF2(s). Ksp = 1.3 x 10-6 if applicable.
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- In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.A student investigates the enthalpy of solution, ΔHsoln for ammonium chloride, NH4Cl. In addition to the salt, the student has access to a calorimeter, a balance with a precision of ±0.1 g, and a thermometer with a precision of ±0.1°C. To measure ΔHsoln for NH4Cl, the student adds 904.0 g of water, initially at 31.0 °C to a calorimeter and adds 155 g of NH4Cl (s), stirring to dissolve. After the NH4Cl dissolves completely, the temperature of the solution is 90.0 °C. Assume the calorimeter was perfectly insulated and the specific heat of the solution was 4.2 J/(g·K). (a) Calculate the q for the dissolving of NH4Cl in water. Include units and proper sign in your answer. Show all work. (b) Calculate the ΔHsoln for NH4Cl, in kJ/molrxn. Include units and proper sign in your answer. Show all work. (c) Is the dissolving of NH4Cl endothermic or exothermic? Justify your answer.Pennies made before 1982 are made of 95% copper. Pennies made after 1982 are made of 97.5% zinc. Look up the heat capacities of Zinc and copper with Google and pick the correct values below a) Zn = 0.388 J/g°C and Cu 0.385 J/g°C b) Zn = 1.388 J/g°C and Cu 0.385 J/g°C c) Zn = 0.388 J/g°C and Cu 1.385 J/g°C d) Zn = 3.388 J/g°C and Cu 2.385 J/g°C
- The internal energy, E, of a system is the sum of the kinetic and potential energy of all of components of the system. What is ΔE (in kJ) for a gaseous system that increases the kinetic energy of it particles using 9,904. J of heat from surroundings and changes the potential energy by doing 5.38 kcal of work against the atmosphere at the same time? (Enter your answer with the correct sign and with two decimal places and no units.) {Hint: be cautious of the signs of the values and units; recall 1 cal = 4.184 J. }2C8H18(l) + 25 O2(g) = 16 CO2(g) + 18 H2O(l) The standard enthalpy of formation for H2O(g)is −241.82kJ/mol The standard enthalpy of formation for CO2(g)is −393.5kJ/mol The standard enthalpy of formation for C8H18(l) is −249.9kJ/mol 1)how much CO2 is released from 1 tank of gas? 2) there are 3000 students and employees. Further assume that they all drive, and on an average they consume 1 tank of gas each, every week to get to and from work. If every tank is 12 gallons (1 gallon = 3.785 L) can you estimate how much heat is transferredYou are camping and need to cook all your food using your camp stove which runs off of propane.If you wanted to warm up your giant mug (67.628 fluid ounces) of morning coffee from 10°C to 80°C,what mass of propane would you have to use?The ΔHcomb for propane is -2219.2 kJ/mol, the density of coffee is 1.0002 g/mL, and the specific heatcapacity of coffee is equal to that of water.1 fluid ounce = 0.0295735 L
- Several ice cubes (ρi = 0.9167 g/cm3) of total volume Vi = 205 cm3 and temperature 273.15 K (0.000 °C) are put into a thermos containing Vt = 680 cm3 of tea at a temperature of 313.15 K, completely filling the thermos. The lid is then put on the thermos to close it. Assume that the density and the specific heat of the tea is the same as it is for fresh water (ρw = 1.00 g/cm3, c = 4186 J/kgK). a. Calculate the equilibrium temperature TE in K of the final mixture of tea and water. b. Calculate the magnitude of the total heat transferred QT in J from the tea to the ice cubes.Suppose we combust a 0.794 g sample of hexane (C6H14, molar mass = 86.18 g/mol) in a bomb calorimeter in the presence of oxygen. If the temperature increase of the calorimeter is 4.08 ºC and the heat capacity of the calorimeter is 9.36 kJ/ºC, calculate the energy of combustion per mole of hexane (ΔH). Show all work and report your answer to the correct units and significant figures.An important flavor component of vanilla extract is vanillin (C8H8O3, molar mass = 152.15 g/mol). When vanillin burns in a bomb calorimeter with a heat capacity of 7.87 kJ/°C, the temperature increases from 25.52°C to 30.43°C. If the heat of combustion of vanillin is -3,760 kJ/mol, what mass of vanillin (in g) was combusted? Please give your answer to 2 decimal places.
- 5 If a 71.98 kg person ate 178 calories worth of sugar (about the calories in a typical energy drink and they converted all of that energy to heat immediately, what would be the change in temperature of that person? A couple of useful facts for this problem. Food calories are actually kilocalories. 1.000 kilocalorie = 4184 JouleWe will assume that the average specific heat of this person's body is 3.00 J/gºC.Enter your answer in ºC with at least 2 sig figs. Just so you are not afraid to eat or drink things, a healthy body is very good at regulating temperature- the bad news is that unless you use it right away, our bodies are very good at converting sugar into fat.A 51−kg person drinks 4.6 × 102 g of milk, which has a caloric value of approximately 3.0 kJ/g. If only 17 percent of the energy in milk is converted to mechanical work, how high (in meters) can the person climb based on this energy intake? Enter your answer in scientific notation.Hint: The work done in ascending is given by mgh, where m is the mass (in kg), g is the gravitational acceleration (9.8 m/s2), and h is the height (in meters).The air in an inflated balloon (defined as the system) is warmed over a toaster and absorbs 130 JJ of heat. As it expands, it does 75 kJkJ of work. What is the change in internal energy for the system? Express your answer using two significant figures.