11) How many KJ of energy would be \'released when condensing 10.00 moles of nit
ID: 1085087 • Letter: 1
Question
11) How many KJ of energy would be 'released when condensing 10.00 moles of nitrogen gas ? [The boiling poi s in the nt for liquid nitrogen atmosphere(25°C and 1.00atrn) into liquid nitrogen (d-0.807g/ml) at 60K is 77x and has a 4H-552k/mol, the molar hat capacity of nitrogen in the gas phase is 29 the liquid phase has a specific heat capacity of 2.042 ng °C)) (lecture slide question) 29.124 /(mol K) and a. -125.3 KJ b. -68.24 K c. -212.42 KJ d. -18.55 KJ 12) What is the Gibbs energy at 298K of the reaction in terms of hydro cyanic acid [Balance ran and use thermo info on last page]: a. -119.1 kJ/mol b. 82.4 ki/mol c. -675.9 k/mol d. 494.0 k/mol 13) How much water will boil when a 193.0g piece of metal at 224°C with .782ng K) is put in a cup of 25.0ml of water at 20.0 a. b. c. d. 24.7g of water boils 11.52 g of water boils 4.82 g of water boils Og of water boils 14) At the equilibrium point of manganese hydroxide in water, how many moles of hydroxide ions will be present in 25ml of water? KalMn(OH),-1.61x10-13) a. 1.23x10" moles OH b. 2.64x10s moles OH c. 1.71x10 moles OH d. 7.4x10 moles OH 15) Calculate H for this reaction: 5 Olg) + 4 NHIg)-> 4 NO(g) + 6 H2O(g) given: &H; = 180.5 kJ/mol &H; =-91.8 k /mol -483.6 kJ/mol a. b. c. d. N2 (g) + O2 (g) 2 NO (g) N2 (g) + 3 H2 (g) 2 NH3 (g) 2H2 (g) +02 (g) 2 H2O(g) -852.5 KJ/(mol NO) -226.5 KJ/(mol NO -143.5 KJ/(mol NO) -522.5 KJ/(mol NO)Explanation / Answer
11
Heat change = mass * specific heat * change in temperature
q1 = 10.0 * 0.029124 * ( 77 - 298)
q1 = - 64.36 kJ
q2 = enthalpy of condesation = 10.00 * 5.52 = - 55.20 kJ
q3 = 10.00 * 0.05718 * (60 - 77)
q3 = - 9.72 kJ
Therefore,
Total heat change = - 64.36 - 55.20 - 9.72 = - 129.28 kJ
So, the answer is (a)
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