1 mol = 22.4L at STP.
Part A: mole = 3.5 moles
Volume = 3.5 X 22.4 = 78.4 L N2 gas.
Part B: Volume = 2.1 L
Mole = 2.1 / 22.4 = 9.375 X 10^(-2) = 0.09375 mol
(3.38). Heat, Q = mC(dT) ; where m = mass in g, C = specific heat and dT = change in temperature.
Part A: m = 95g, Ti = 45°C, Tf = 29°C and C = 1 cal/g-°C.
Heat lost = -95 X 1 X (29-45) = 1520 cal.
Part B: m = 21g, Ti = 86°C, Tf = 62°C and C = 4.184 J/g-°C.
Heat Lost = -21 X 4.184 X (62 - 86) = 2108.74 J
Part C: m = 4.8 kg, Ti = 22°C and Tf = 24°C.
Heat = 4.8 X 1 X (24-22) = 9.6 kCal.
Part D: m = 225g = 0.225 kg, Ti = 18°C and Tf = 175°C
Heat = 0.225 X 4.184 X (175-18) = 147.8 kJ.
A Revi Use molar volume to calculate each of the following at STP: Part A the...
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Please answer in detail on how these 2 answers are gotten. Include Heat formula (or any formula) and all math used to get to answer Calculate the mass, in grams, for each of the following using the table below Table Specific Heats of Some Substances Specific Heat (J/g C) Substance Aliminium, Al(s) Copper, Cu(s) Gold, Au(s) ron, Fe(s) Silver. Ag(s) Titanium, Ti(s) 0.897 0.385 0.129 0.452 0.235 0.523 2.04 2.46 0.864 4.184 2.03 Elements Compounds Ammonia, NHs(g) Ethanol, C2H5OHl) Sodium...
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