Al(s) + ClO (aq) A10, (aq) + Cl(aq) Express your answer as a lonic equation. Identify all of the phases in your answer.

The vapor pressures of the components, A and B, in a binary solution have been modeled and found to obey PA = XAPA* exp(XB²) PB = XBPB* exp(X₁²) A where ΧΑ and XB are the mole fractions, and PA* and PB* are the vapor pressures of each pure substance. (a) If PA* = 0.175 bar and PB* = 0.126 bar, compute the total vapor pressure (in bars) of the mixture when XB XB = 0.68. (b) Assuming that the vapor is an ideal gas, what are the mole fractions of each component in the vapor phase?

The vapour pressure of a liquid between 15 °C and 35 °C fits the expression log(p/Torr) = 8.750 − (1625 K)/T. Calculate (i) the enthalpy of vaporization and (ii) the normal boiling point of the liquid.

The vapour pressure of a substance at 20.0 °C is 58.0 kPa and its enthalpy of vaporization is 32.7 kJ mol−1. Estimate the temperature at which its vapour pressure is 66.0 kPa.

Assuming 100% dissociation, calculate the freezing point (T) and boiling point (T,) of 2.23 m Na, SO, (aq). Colligative constants can be found in the chempendix. T = T =

Assume you are interested in exploring the use of ammonium nitrate (NH4NO3) as the active ingredient in an inexpensive home-made cold pack. You decide that a practical cold pack should be able to depress the temperature of 1 kg of human muscle tissue by 5 oC. Now you need to know the amount of NH4NO3 required to achieve this. Ammonium nitrate is a highly water soluble solid. You believe the enthalpy of dissolution  for NH4NO3 must be determined. To this end, you add 2.339 g of NH4NO3 to 99.7 mL of water at 23.7 °C in a constant-pressure calorimeter and close the calorimeter. The temperature of the water decreases to a minimum of 21.9 °C. 1a. Assume the density and specific heat of water is 1.00 g/mL and 4.184 J/g °C, respectively. Using the data above, determine the  for ammonium nitrate in water. Assume the heat capacity of the calorimeter is negligible.

Assume you are interested in exploring the use of ammonium nitrate (NH4NO3) as the active ingredient in an inexpensive home-made cold pack. You decide that a practical cold pack should be able to depress the temperature of 1 kg of human muscle tissue by 5 oC. Now you need to know the amount of NH4NO3 required to achieve this. Ammonium nitrate is a highly water soluble solid. You believe the enthalpy of dissolution  for NH4NO3 must be determined. To this end, you add 2.339 g of NH4NO3 to 99.7 mL of water at 23.7 °C in a constant-pressure calorimeter and close the calorimeter. The temperature of the water decreases to a minimum of 21.9 °C 1) The specific heat of human muscle tissue (smuscle) is 3.47 kJ/kg oC. Given this value, how many grams of ammonium nitrate (NH4NO3) is required to depress the temperature of 1.00 kg of human muscle by 5.00 oC? Please remember, show all work in a legible, highly organized manner

Enter a net ionic equation for the reaction of acetic acid, CH3COOHCH3COOH, with zinc. Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.