A mixture of 20.6g of phosphorus (P) and 79.4 chlorine (Cl2)
reacts completely to form phosphorus trichloride (PCl3) and
phosphorus pentachloride (PCl5).
(a) true or false: the bond angels of PCl3 and PCl5 are
identical.
(b) what mass of PCl3 forms under the conditions described
above?
(c) an analysis of a phosphorus and chlorine containing compound
found that it was 30.40% phosphorus. is it one of the two products
formed in this reaction? why pr why not?
A 5 g mixture of ethanol (C2H5OH) and
methanol (CH3OH) reacts with excess oxygen. If this
combustion releases 125.46 kJ of heat, what mass of ethanol is in
the mixture? Assume that mixing does not affect any enthalpy
values.
C2H5OH(l) + 3 O2(g) --> 2
CO2(g) + 3 H2O(g)
-277.63
-393.5 -241.83 (kJ/mol)
CH3OH(l) + 1.5 O2(g) -->
CO2(g) + 2 H2O(g)
-201.2
-393.5 -241.83 (kJ/mol)
A mixture of LiAlH4 and LiCl weighs 7.51 g. LiAlH4 reacts
exothermically with ethanol according to the following equation
LiAlH4(s) + 4CH3CH2OH(l) → Li[Al(OC2H5)4](s) + 4H2
14.48 g of Li[Al(OC2H5)4] is formed when this sample is
dissolved in CH3CH2OH, what percentage of the original sample is
LiAlH4, also what percentage is LiCl? Assuming LiAlH4 is completely
turned into Li[Al(OC2H5)4] and LiCl dissolves in ethanol
How many grams of product form when 17.8 g of O2 reacts
completely? (Assume you have enough Cr) Chromium solid reacts with
oxygen gas to form chromium (III) oxide How many moles of Cr(s) is
needed for 17.8 g of oxygen gas to react completely
Iron(III) oxide reacts with carbon monoxide according to the
equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 22.25 g Fe2O3and 14.18 g
CO.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant is left?
Iron(III) oxide reacts with carbon monoxide according to the
equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 23.00 g Fe2O3 and 16.00 g
CO.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant is left?
(Sig Figs) Iron(III) oxide reacts with carbon
monoxide according to the equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 22.20 g
Fe2O3 and 14.00 g CO.
The online website said the answer is m = 2.32g ( 3 sig
figs)
While my answer was 2.318 ( 4 sig figs)
Heres my calculations
22.20 g Fe2O3 / 159.69 =
0.13901934999060680067631035130565 mols of
Fe2O3
14.00 g CO / 28.01 = 0.49982149232416993930739021777936 mols
of CO
0.13901934999060680067631035130565 x 3 =
0.41705804997182040202893105391696 mols of
Fe2O3 needed to...
Iron(III) oxide reacts with carbon monoxide according to the
equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 22.90 g Fe2O3 and 15.78 g
CO.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant is left?
Iron(III) oxide reacts with carbon monoxide according to the
equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 22.10 g Fe2O3 and 14.00 g
CO.
Once the reaction has occurred as completely as possible, what
mass (in g) of the excess reactant remains?
Express your answer to three significant figures.
Suppose that in an alternate universe, the possible values of
l were the integer values from 0 to n(instead of
0 to n−1). Assuming no other differences from this
universe, how many...
1.The total pressure of a mixture of O2(g) and H2(g) is 1.95
atm. The mixture is ignited and the resulting water is removed. The
remaining mixture is pure H2(g) and exerts a pressure of 0.210atm
when measured at the same temperature and volume as the original
mixture. What were the mole fractions of O2(g) and H2(g) in the
original mixture?