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
Knowing that Delta H vap for water is 40.7 Kj/mol calculate Pvap (vapor pressure) of water...
Knowing that delta H of water is 40.7 Kj/mol How many KJ will be required to vaporize 50.0 g of water? Calculate the percent error if you obtain a value of 39.2 Kj/mol for delta h vap for water for experiment
1. An espresso maker can put a pressure of 9.0 atm on water. Given (Delta ) H Vap(H20) Determine the boiling point of water in it in C. = 40.7 kJ/mol.
The vapor pressure of the liquid HF is measured at different temperatures. The following vapor pressure data are obtained: Temperature 270.6K and 287.5K, Pressure 324.5 mmHg and 626.9 mmHG. Calculate the enthapy of vaporization ( delta H vap ) in kJ/mol for this liquid.
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.
1)2)1)The vapor pressure of ethanol is \(1.00 \times 10^{2} \mathrm{mmHg}\) at \(34.90^{\circ} \mathrm{C}\). What is its vapor pressure at \(63.16^{\circ} \mathrm{C}\) ? ( \(\mathrm{AH}_{\text {vap }}\) for ethanol is \(39.3 \mathrm{~kJ} /\) mol. )\(\mathrm{mmHg}\)2)Calculate the amount of energy (in kJ) necessary to convert \(457 \mathrm{~g}\) of liquid water from \(0^{\circ} \mathrm{C}\) to water vapor at \(187^{\circ} \mathrm{C}\). The molar heat of vaporization \(\boldsymbol{H}_{\mathrm{vap}}\) ) of water is \(40.79 \mathrm{~kJ} / \mathrm{mol}\). The specific heat for water is \(4.184 \mathrm{~J} /...
Calculate the enthalpy change, Delta H process in which 32.5 g water is converted from liquid at 18.9 C to vapor 25.0 degrees C. For water Delta H vap =44.0 kJ/mol at 25.0 °C and Cs=4.18 J/(g*^ C) for H2O (l)
Question 6 Calculate the vapor pressure of water at 52.4°C in units of torr. The enthalpy of vaporizatio water is 40.7 kJ/mol. The normal boiling point of water is 100°C. No new data to save. Last checked at 2:02pm
The standard enthalpy of vaporization (H°vap) of carbon tetrachloride (CCl4) is 34.6 kJ/mol. The normal boiling point of carbon tetrachloride is 76.5°C. Calculate the vapour pressure of carbon tetrachloride at 62.5°C. after solving I got 0.4994 when using Clausius - Clapeyron equation. How do I get P2?
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...
The vapor pressure of water is 1.0 atm at 373 K, and the enthalpy of vaporization is 40.7 kJ mol-1 . At what temperature will the vapor pressure be 0.697 atm and at what temperature will the vapor pressure be 1.409 atm?