SBCH1103: Calculate the pressure exerted by 0.0153 moles of CO2 gas in a container of 1.467 L  at 20.0°C: Inorganic Chemistry Assignment, OUM, Malaysia

Question 1

a) Calculate the pressure exerted by 0.0153 moles of CO2 gas in a container of 1.467 L  at 20.0°C.

b) What is the volume of a 15.0 g sample of propane (C3H8) gas at Standard Temperature Pressure?

c) Assuming that the volume of the container part (b) above remains constant, what would be the pressure of the propane at room temperature (25 °C)?

d) A 1.00 g gaseous sample of hydrocarbon occupies a volume of 385 mL at 330 K and 1.00 atm. Find the molar mass of the compound.

e) Calculate the number of atoms of He(g) that are needed to exert a pressure of 4.0 atm in a 15 mL container at a temperature of     –23°C.

Question 2

a) 200.0 g of Ca(C2H3O2)2 was found in the chemistry laboratory.

Calculate
i.  the molecular mass of 1 mole Ca(C2H3O2) 2.

the number of moles of Ca(C2H3O2)2  that exists
iii.  the number of Ca(C2H3O2)2 molecules present

the volume at STP  if Ca(C2H3O2)2 is converted to gas.
v.   the molarity of a solution made by dissolving 200.0 g of

Ca(C2H3O2)2 in 200 ml of water

b) Answer the following stoichiometry questions by referring to the equation below:

KClO3 2 KCl + 3 O2

If 1.50 moles of KClO3 decompose, what is the mass of O2 that will be produced?

If 80.0 grams of O2 were produced, how many moles of KClO3   are decomposed?

Find the mass of KClO3  needed if we need to produce 2.75 moles of KCl.

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