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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.111.1Ms = ? ks show work, report sig figs and unitsThe answer for this is 25.9 j/°c but I dont know how to get it. Pls tell me
- Element X has an enthalpy of fusion of 59.2 kJ mol-1 at its melting point (684°C). Calculate ΔSsys for the process,X(l) → X(s)At 1 bar and 684°C. Express your answer in units of J mol-1 K-1 to 3 significant figures.In a generic chemical reaction involving reactants A and B and products C and D, aA+bB→cC+dD, the standard enthalpy ΔH∘rxn of the reaction is given by ΔH∘rxn=cΔH∘f(C)+dΔH∘f(D) −aΔH∘f(A)−bΔH∘f(B) Notice that the stoichiometric coefficients, a, b, c, d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right-hand side of the equation is a sum over the products and the second sum is over the reactants: ΔH∘rxn=∑productsnΔH∘f−∑reactantsmΔH∘f where m and n represent the appropriate stoichiometric coefficients for each substance. What is ΔH∘rxnΔHrxn∘ for the following chemical reaction? CO(g)+NH3(g)→HCN(g)+H2O(g) You can use the following table of standard heats of formation (ΔH∘f)(ΔHf∘) to calculate the enthalpy of the given reaction. Element/ Compound Standard Heat of Formation (kJ/mol) Element/ Compound Standard Heat of Formation (kJ/mol) H(g) 218218 N(g) 473473 H2(g) 00 O2(g) 00 NH3(g) −45.90 O(g) 249 CO(g)…A 43.97 kg cheetah is running after a gazelle at 24.89 m/s What is the kinetic energy of this cheetah in joules while chasing the gazelle at this rate of speed?
- To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.The DHvap of ethanol is 33.9 kJ/mol and its boiling point is 78.3 °C. Calculate the DSvap in J/K of 3.00 moles of ethanol. Write the correct equation that is used, and plugging in the correct numbers with the correct units.Let temperature in 3-space be given by T (x, y, z) = x2 + y2 - z.Draw isotherms corresponding to temperatures T = - 2, -1, 0, 1, 2.
- [tot] Mn(s) + O2(g) → MnO2(s) ΔH(tot) = ___________? [1] 2MnO2(s) → 2MnO(s) + O2(g) ΔH1 = +264 kJ [2] MnO2(s) + Mn(s) → 2MnO(s) ΔH2 = –240 kJ [tot] = __×[1] __×[2]: ________________→________________ ΔH(tot) = __×ΔH1 __×ΔH2 = ______________kJThe amount of heat (q) gained or lost by a substance (with mass m) as its temperature changes (ΔT) depends on its specific heat capacity (Cp) according to the following equation. q = Cp ✕ m ✕ ΔT The quality of industrial diamonds is determined in part by measuring the specific heat capacity, which is 0.5091 J/g·K for pure diamond. If the absorption of 26.06 J of heat by a 2.10 g diamond sample of unknown purity causes its temperature to rise from 25.90°C to 73.45°C, is the diamond sample pure? Explain your reasoning. The calculated Cp is ____________________ J/g·K and the value for pure diamond is 0.5091 J/g·K. These values are (fairly close or equal/significantly different) , thus the sample (is/is not) pure.Consider the two spheres shown here, one made of silver andthe other of aluminum. (a) What is the mass of each spherein kg? (b) The force of gravity acting on an object is F = mg,where m is the mass of an object and g is the acceleration ofgravity (9.8 m/s2). How much work do you do on each sphereit you raise it from the floor to a height of 2.2 m? (c) Does theact of lifting the sphere off the ground increase the potentialenergy of the aluminum sphere by a larger, smaller, orsame amount as the silver sphere? (d) If you release thespheres simultaneously, they will have the same velocitywhen they hit the ground. Will they have the same kineticenergy? If not, which sphere will have more kinetic energy?[Section 1.4]
