Chemistry Answers

A solution is made by dissolving 75.0 grams glycerin C3H803 (92 g/mol), in 600.0 grams of water (18 g/mol) to make approximately 600 -mL solution. Calculate the following:

a. Vapor pressure of the solution at 25.0 Celsius (The vapor pressure of pure water is 23.8 torr at 25.0 Celsius).

b. Boiling point of the solution

c. Freezing point of the solution

d. Osmotic pressure at 25.0 Celsius

CH4

The reaction of 1.00 mol of solid phosphorus with chlorine gas to form PCl3(g) releases 287.0 kJ of heat energy. The reaction of 1.00 mol of solid phosphorus with chlorine gas to form PCl5(g) releases 374.9 kJ of heat energy. Using Hess’s law, indirectly calculate the enthalpy change (in kJ.mol-1 ) for the following reaction.

What percentage of oxygen is present in the compound CaCO3.3Ca3(PO4)2? (A) 23.3% (B) 45.36% (C) 41.94% (D) 17.08%  

What is Studies fundamental concepts

What volume of carbon (IV) oxide in dm 3 is produced at s.t.p. when 2.50g of CaCO3 reacts with excess acid according to the following equation? CaCO3(s) + 2HCI(aq) → CaCl2(aq) + H2O(1) + CO2(g)[CaCO2 100; molar volume of a gas at s.t.p. = 22.4dm 3]

2.95 g of chloroform, CHCl₃ (119.37 g.mol^-1), is placed in a closed 2.00 L flask at 90 ^oC which contains air whose pressure is 83.0 kPa. the chloroform vaporizes.

1. Calculate the partial pressure of chloroform.
2. Find the total pressure and mole fraction of the chloroform.

Consider the equilibrium reaction: 2NO (g) + O₂ (g) ⇌2NO₂ (g) Δ_rH = -114 kJ.mol^-1

1. With a gas mixture comprising of 20% mole each of NO and NO₂, the remainder being O₂, and K_p = 9.0 at 298 K.
2. Deduce the pressure at which the mixture is at equilibrium

The s and f sub-levels contain electrons for

How many grams of water can react with 7.30 moles of carbon dioxide