Determine delta H(vap) for a molecule with a Vapor pressure of 25.2 torr at 273 K and 56.2 torr at 295 K.
Determine delta H(vap) for a molecule with a Vapor pressure of 25.2 torr at 273 K...
What is the vap of a liquid that has a vapor pressure of 612 torr at 84.6oC and a boiling point of 96.9oC at 1 atm?
Knowing that Delta H vap for water is 40.7 Kj/mol calculate Pvap (vapor pressure) of water at 37Celsiuse I need to know how this is done i know the answer is 52.5 mmhg
Ethanol has a vapor pressure of 58.3 torr at 25 degree C. Determine the delta H (we assume that delta H in independent of temperature). l_n (p_2/58, 3) = delta / (1/351, 4 - 1/298) A 0.250 g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g of water wend 50.0 g of ice at 0 degree C. The reaction is: 2Na(s) 2H2O) + 2H_2O(l) rightarrow 2NaOH(aq) +H_2(g); delta H = -368 kJ. Will all the...
A certain liquid has a vapor pressure of 92.0 Torr at 23.0 ∘ C and 306.0 Torr at 45.0 ∘ C. Calculate the value of Δ H ∘ vap for this liquid. Δ H ∘ vap = kJ / mol Calculate the normal boiling point of this liquid. boiling point: = ∘ C
A certain liquid has a vapor pressure of 92.0 Torr at 23.0 ∘C and 273.0 Torr at 45.0 ∘C. 1)Calculate the value of Δ?∘vap for this liquid. Δ?∘vap= kJ/mol 2)Calculate the normal boiling point of this liquid.
What is the ΔH o vap of a liquid that has a vapor pressure of 616 torr at 81.8°C and a boiling point of 93.8°C at 1 atm?
A substance has a vapor pressure of 600 torr at 85 degree C. Its delta H_vap is 31.3 kJ/mol. What is its vapor pressure at 25 degree C?
3. (5 pts) Carbon tetrachloride has a vapor pressure of 11.3 torr at 255 K, and 99,0 torr at 295 K. What is the normal boiling point in °C) of carbon tetrachloride? 4. (5 pts) At its boiling point, how much heat would be required to vaporize 225.0 mL of carbon tetrachloride? pcc = 1.59 g/cm".
A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 226.0 Torr at 45.0 °C. Calculate the value of ΔH°vap for this liquid. Calculate the normal boiling point of this liquid.
The vapor pressure of ethanol is 115 torr at 34.9 oC and ΔHvap of ethanol is 38.6 kJ/mol, use this information and the Clausius-Clapeyron equation (shown below) to calculate the temperature in oC at which the vapor pressure is 760 torr (remember to convert temperatures to K in the equation (K = oC + 273). R = 8.314 J/mol·K. ( Please show each step, step BY step) I am having difficult with finding T2