Calculate w and ΔE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The ΔH vaporization is 39.9 kJ/mol at 265 K.
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Calculate w and ΔE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and...
ZnC4H10 is liquid that spontaneously undergoes combustion in the presence of air according to the following equation ZnO (s) + CO2 (g) ZnC4H10 (1) + O2 (g) + H2O (g) 1. Balance the equation. 2. Calculate w and AE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The AH vaporization is 39.9 kJ/mol at 265 K.
ZnC4H10 is liquid that spontaneously undergoes combustion in the presence of air according to the following equation ZnC4H10 (l) + O2 (g) ---> ZnO (s) + CO2 (g) + H2O (g) Balance the equation. Calculate w and Δ E when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The Δ H vaporization is 39.9 kJ/mol at 265 K.
Please show all work and explanations! Calculate ΔE, ΔS, ΔG, Q and W for the vaporization of 3.00 moles of liquid water to form water vapor at 100°C and 1.00 atm pressure. The standard molar enthalpy of vaporization of water is 40.67 kJ/mol. The density of liquid water at 100°C is 0.958 g/cm3 . Assume that the water vapor is an ideal gas, but be careful – the initial state is liquid water, so this is not simply an ideal...
1) The vapor pressure of liquid antimony is 400 mm Hg at 1.84×103 K. Assuming that its molar heat of vaporization is constant at 115 kJ/mol, the vapor pressure of liquid Sb is _____ mm Hg at a temperature of 1.81×103 K. 2) The normal boiling point of liquid acetone is 329 K. Assuming that its molar heat of vaporization is constant at 29.0 kJ/mol, the boiling point of CH3COCH3 when the external pressure is 1.21 atm is ______ K.
For ammonia, ΔHvap = 23.6 kJ/mol at its boiling point, -33 oC. Calculate the values for ΔS, q, w, and ΔE for the vaporization of ammonia at -33 oC and 1 atmosphere pressure.
The vapor pressure of liquid antimony is 400 mm Hg at 1.84x108 K. Assuming that its molar heat of vaporization is constant at 109 kJ/mol, the vapor pressure of liquid Sb is mm Hg at a temperature of 1.87X10 K.
1.000 mol of ammonia is vaporized at a constant pressure of 1.000 atm and a constant temperture of 240 K, the normal boiling temperture. The enthalpy change of the vaporization at this temperture is 25.11 kJ/mol. Find delta G, delta S, w and q.
The vapor pressure of liquid nickel is 400 mm Hg at 2.89×10³ K. Assuming that its molar heat of vaporization is constant at 410 kJ/mol, the vapor pressure of liquid Ni is mm Hg at a temperature of 2.93×10³ K. Submit Answer
36.1 J/K mol. Calculate the boiling point of liquid Liquid nitrogen has a measured enthalpy of vaporization (AH vap -2.79 kJ/mol and entropy of vaporization (AS nitrogen, in °C using this information. (Use 273.15 K 0°C for the temperature conversion. Report your answer with three significant figures.) Tp C
The vapor pressure of liquid antimony is 400 mm Hg at 1.84x10' K. Assuming that its molar heat of vaporization is constant at 115 kJ/mol, the vapor pressure of liquid Sb is m m Hg at a temperature of 1.81x10' K.