tutorial chapter 1: solutions

chapter 1

1.		Sodium hydrogen carbonate is prepared from NaCl and ammonium hydrogen carbonate, according to equation: NH4HCO3(aq)  +  NaCl (aq)    ®  NaHCO3 (aq)  +  NH4Cl (aq) If 0.3 mol NH4HCO3 are reacted with 0.2567 mol of NaCl, how many grams of NaHCO3 are obtained?
2.		CH4 (g)  +  H2O (g)  ®  3H2 (g)  +  CO (g) What mass of H2O is required to react exactly with 249 g of methane?
3.		Suppose 25.0 kg of nitrogen gas and 5.00 kg of hydrogen gas are mixed and reacted to form ammonia. Calculate the mass of ammonia produced when this reaction is run to completion.
4.		Balance these two equations below:
	a)	Na   +   H2O   ­®   NaOH   +   H2
	b)	NH4OH   +   H2SO4   ­®   (NH4)2SO4   +   H2O
5.		When aluminium metal is exposed to air, a protective layer of aluminium oxide (Al2O3) forms on its surface. This layer prevents further reaction between aluminium and oxygen, and it is the reason that aluminium beverage cans do not corrode. [in the case of iron, the rust or the iron(III) oxide, that forms is too porous to protect the iron metal underneath, so rusting continues]. Write a balanced equation for the formation of Al2O3
6.		Balance the equation representing the reaction between iron(III) oxide, Fe2O3, and carbon monoxide (CO) to yield iron (Fe) and carbon dioxide (CO2)
7.		Balance the following equations.
	a)	NaOH   +   H2SO4   ­®   Na2SO4   +   H2O
	b)	N2O5   ­®   N2O4   ­®   O2
8.		Urea [(NH2)2CO] is prepared by reacting ammonia with carbon dioxide: 2NH3 (g)   +   CO2 (g)   ­®   (NH2)2CO (aq)   +   H2O (l) In one process, 637.2 g of NH3 are treated with 1142 g of CO2.
	a)	Which of the two reactants is the limiting reagent?
	b)	Calculate the mass of (NH2)2CO formed.
	c)	How much excess reagent (in grams) is left at the end of the reaction?