Search & Filtering
A reaction to convert ammonia into nitric acid involves the following chemical equation:
4 NH3 (g) + 5 O2 (g) 4 NO(g) + 6 H2O(g)
Assume that 1.50 g of NH3 reacts with 2.75 g O2.
i. Determine the limiting reactant.
ii. Calculate how many grams of NO and H2O will form in the reaction above.
iii. Calculate how many grams of the excess reactant will remain after the reaction is complete.
iv. If the yield obtained for NO is 1.80 grams and yield obtained for H2O is 1.50 grams, calculate the percent yield of NO and H2O in this reaction.
(Atomic mass of N = 14 ; O = 16 ; H = 1)
Explain why pentane is insoluble in water
Calculate the total amount of energy (in kJ) necessary to raise the temperature of 2.00 L of ethanol (density
= 0.7849 g/cm3
) from 18 0C to its boiling point (78.3 0C) and then to fully vaporize the liquid. Assume that
it is a closed system where no heat exchange with the surroundings take place.
(Given: Cethanol = 2.44 J/g·K; heat of vaporization of ethanol at 78.3 0C = 38.56 kJ/mol.)
[5 marks)
A water soluble salt is reacted separately with HCl, H SO and NaOH and form precipitates. When this salt is 2 4
heated thoroughly a black residue is formed liberating a gas. The salt is,
Explain the following: a} Why does increasing the temperature cause a substance to change in succession from a solid to a liquid to a gas? b) Explain why a liquid has a definite volume but a gas does not? c) Discuss how does an amorphous solid differs from a crystalline solid? d) Explain with examples, how bonds are termed in ionic compounds and covalent compounds. e)Covalent bonding occurs in both molecular and covalent network solids. Why do these two kinds of solids differ so greatly in their hardness and melting points?
A reaction to convert ammonia into nitric acid involves following chemical equation:
4 NH3 (g) + 5 O2 (g)à 4 NO(g) + 6 H2O(g)
Assume that 1.50 g of NH3 reacts with 2.75 g O2, then:
1. Determine the limiting reactant
2. Calculate how many grams of NO and H2O will form in the reaction above
3. Calculate how many grams of the excess reactant will remain after the reaction is complete.
4. If the yield obtained for NO is 1.80 grams and yield obtained for H2O is 1.50 grams, calculate the percent yield of NO and H2O in this reaction.
(Atomic mass of N = 14 ; O = 16 ; H = 1).
Calculate each of the following quantities for an ideal gas: a) The volume of the gas in litre, if 2.57 moles have a pressure of 1.86 atm at a temperature of -12ºC. b) The absolute temperature of a gas at which 6.79 X 10 2 moles occupies 164 ml at 893 torr. c) The pressure in atm , if 8.25 X 10 2 moles occupies 255 mL at 15°C. d) If oxygen gas is used, calculate the mass of the oxygen gas in grams, if 5.49 L at 45ºC has a pressure of 11.25 kPa.
If 0.007 g of KHP (molar mass = 204.23) requires 30.0 mL of NaOH upon titration, what is the normality of NaOH?
Given four 250-mg tablets of aspirin (90% purity), what volume of 0.50 N NaOH is used in the hydrolysis reaction if 10.00 mL of 0.50 N HCl is consumed in the back titration?
It is known that 35.00 mL of an acid solution is needed to titrate 38.50 mL of a base solution. What is then the volume relationship of the two solutions?
