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At 35.0 oC, the vapor pressure of chloroform is 295.1 torr and that of ethanol is 102.8 torr. a. Which of these liquids has the higher boiling point? b. A chloroform-ethanol solution at 35 oC with ?ethanol=0.200 in the liquid phase has a vapor pressure of 304.2 torr and a vapor composition of Yethanol= 0.138. Calculate the activity and activity coefficient for ethanol in this solution. c. Calculate ?mixG for a solution that contains 0.12 moles of ethanol and 0.83 moles of chloroform at 35.0 oC.
What is the molarity of the resulting solution when 28.249 g of Mn(ClO4)2 · 6 H2O are added to 550.0 mL of water?
The solubility of O2 (g) in water is 4.43mg O2/100 g H2O (20ºC and 1 atm). What is the molarity (M) of this saturated solution?
calculate the number of tons of carbon dioxide and sulfur dioxide produced by the plant during the year. (b) If 55% of SO2 could be removed by reaction with powdered CaO to form CaSO3, how many tons of CaSO3 would be produced.
PbCO3(s)+2H^+(aq)+2H^+(aq) yields Pb^2++H20(l)+CO2(g), how many grams will dissolve when exactly 4.5 L of 2.00 M H+ is added to 3.00 g of PbCO3
calculate the mass of water that must be added to 0.45 mol of glucose to make a solution of 15.0 percent by mass. the molar mass of glucose is 180 g/mol
Suppose 5.00g of Ca is added to 50.0mL of 1.00M HCL. Determine the limiting reactant in this case and number of moles of calcium actually consumed.
In general, oxides of elements further to the left on the periodic table are basic, moving toward acidic on the right. For nonmetallic oxides, when the oxidation number of the element other than oxygen is high, the oxide tends to be acidic. When t..
To determine the concentration of Cu+2 in a large sample of water an electrochemical was constructed usingAg+1 (1.0 M) and Ag as the athode and Cu in the CU+2 containing solution as the anode. the cell potental was measure to be .62volts. what is t..
The density of titanium metal is 4.51 g/cm}^3 at 25 C}. What mass of titanium displaces 69.6 mL of water at 25 ^C?
how many moles O2 of are present? (The mole fraction of in dry air is 0.2095.) How many grams of C8H18 could be combusted by this quantity of O2
If 37.4 grams of water decomposes at 297 Kelvin and 1.30 atmospheres, how many liters of oxygen gas can be produced? 2 H2O (l) yields 2 H2 (g) + O2 (g)
Consider the following data. 2 Ca(s) + O2(g) 2 CaO(s) H = -1270.2 kJ C(s) + O2(g) CO2(g) H = -393.5 kJ CaO(s) + CO2(g) CaCO3(s) H = -178.3 kJ Use Hess's law to calculate H for the reaction below.
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