Physical Chemistry Answers

Calculate the mass of CO₂ in 2.0L soft drink after the bottle is opened and equilibrates at 25°C under a CO₂ partial pressure of 3.0×10^-4 atm.The Henry's law constant for CO₂ at this pressure is 3.4×10^-2 mmolL.atm

Consider the following reaction:

H2O(g) + CO(g) H2(g) + CO2(g)

The equilibrium constant Kp for this reaction is 0.55 at 1023 K.

(i) In a reaction vessel, water vapour and carbon monoxide are introduced at a pressure of 3.50 atm, and allowed to reach equilibrium at 1023 K. Construct a table and use it to calculate the partial pressure of all the gases at equilibrium.

explain the Bi- cd system

A sample of water was alkaline both to phenolphthalein and methyl orange. 100 mL of this water sample required 20 mL of N/50 HCl for phenolphthalein end point and another 15 mL for complete neutralization. Elucidate the type and strength of alkalinity present in the water sample

one mole of an ideal gas is allowed to expand at 25 degree celsius till its pressure falls to one- fifth of its original pressure. find out the free energy

H3PO4 sample (M.Wt =98) if 0.5 M NaOH used as a titrant. find the concentration

Does a precipitate form if you add 15.00 𝑚𝐿 of a 2.10 × 10−3 𝑚𝑜𝑙/𝐿 solution of lead (II) nitrate to 25.00 𝑚𝐿 of a 2.50 × 10−2 𝑚𝑜𝑙/𝐿 solution of potassium chloride? Justify your answer mathematically. (𝐾𝑠𝑝 𝑓𝑜𝑟 𝑙𝑒𝑎𝑑(𝐼𝐼)𝑐h𝑙𝑜𝑟𝑖𝑑𝑒 𝑖𝑠 1.7 × 10−5)

At 150K, bromine gas and chlorine gas combine to form gaseous bromine chloride. Determine the

𝐾𝑃 for the reaction if the partial pressures are as follows.

𝑃 = 1.67 𝑎𝑡𝑚 𝐵𝑟2

𝑃 = 1.42 𝑎𝑡𝑚 𝐶𝑙2

𝑃 = 0.061 𝑎𝑡𝑚

The enthalpy of formation of NH3(g) as per the following reaction is -46.11 kJ/mol at 298 K.

N2(g) + 3H2(g) 2 NH3(g) 

Calculate the value of enthalpy of formation of NH3(g) at 100 oC. The Cp values are given as: N2(g) = 29.12; H2(g) = 28.82; NH3(g) = 35.06. Assume the given heat capacity values to be temperature independent in the range. 

An additional piece of solid CaCO 3 is added to the equilibrium caco3 to its ions

The rate of dissolving and rate of crystallization have increased. Why?