Each of the following elements reacts with oxygen in combus- tion reactions.
Each of the following elements reacts with oxygen in combus- tion reactions. Identify whether the products of these reac- tions would be ionic compounds or covalent compounds.
When the supply of oxygen is limited, iron metal reacts with
oxygen to produce a mixture of FeO and Fe2O3 . In a certain
experiment, 20.00 g iron metal was reacted with 11.31 g oxygen gas.
After the experiment, the iron was totally consumed, and 3.91 g
oxygen gas remained. Calculate the amounts of FeO and Fe2O3 formed
in this experiment.
If 3.50 mol of Fe reacts with 3.00 mol of oxygen in the
following reaction: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) Which of the
following statements is correct? If 3.50 mol of Fe reacts with 3.00
mol of oxygen in the following reaction: 4 Fe(s) + 3 O2(g) → 2
Fe2O3(s) Which of the following statements is correct?
a)Fe is the limiting reactant and 1.75 mol of product can be
produced.
b)O2 is the limiting reactant and 2.00...
What are the stereochemical formula equations for the following
reactions?
(a) propene reacts with hydrogen chloride gas
(b) ethane undergoes complete combustion
(c) butane reacts with bromine
(d) pent-2-ene reacts with water
(e) cyclohexanol eliminates water to produce a cycloalkene
(f) 2-bromopropane undergoes an elimination reaction with
hydroxide ions
(g) ethanol reacts with propanoic acid
Model the equations given above. Include all reactants and all
(primary) products as well as the correct IUPAC name(s) for all
organic products. (You do...
Enter the balanced chemical equation for each reaction.
A. Gaseous hydrogen chloride reacts with oxygen gas to form
chlorine gas and liquid water.
B. Solid iron(III) oxide reacts with hydrogen gas to form solid
iron and liquid water.
C. Nitric oxide gas reacts with hydrogen gas to form ammonia gas
and water vapor.
D. Solid iron(III) oxide reacts with carbon monoxide gas to form
solid iron and carbon dioxide gas.
Ammonia reacts with oxygen to form nitrous monoxide and water as
in the following equation: 4NH3(g) +5O2=4NO(g) + 6H2O(g) How many
liters of H2O gas can be produced given a temperature of 48° c and
a pressure of 975 torr from 145.0 grams of NH3?
In the following reaction, 451.4 g of lead reacts with excess
oxygen forming 321.9 g of lead(II) oxide. Calculate the percent
yield of the reaction. 2Pb(s)+O2(g)-->2PbO(s)
Write balanced net ionic equations for the following reactions
in acid solution.
a. Liquid hydrazine reacts with an aqueous solution of sodium
bromate. Nitrogen gas and bromide ions are formed.
b. Solid phosphorus (P4) reacts with an aqueous solution of
nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4
-) ions.
c. Aqueous solutions of potassium sulfite and potassium
permanganate react. Sulfate and manganese (II) ions are formed.
Write the balanced equations for the following
reactions: States are graded.
Solid white phosphorus, P4(s), reacts with excess
chlorine gas to produce solid phosphorus pentachloride.
Liquid phosphorus trichloride reacts with water to produce
hydrochloric acid and phosphorus acid.
Hydrolysis of solid calcium phsophide produces phosphine gas,
PH3(g) and calcium hydroxide.
The compound P4S3 is used in matches. It
reacts with oxygen to produce P4O10 and
SO2. The unbalanced chemical equation is shown
below:
P4S3(s) + O2(g) -->
P4O10(s) + SO2(g)
What mass of SO2 is produced from the combustion of
0.401 g P4S3?
Consider the following three reactions. For each of the
reactions, use data in Appendix C in the textbook to calculate ΔH∘,
ΔG∘, and ΔS∘ at 25 ∘C.
Calculate ΔS∘ for C2H6(g)+7Cl2(g)→2CCl4(g)+6HCl(g) Express your
answer using three significant figures.
Calculate ΔG∘ for C2H6(g)+7Cl2(g)→2CCl4(g)+6HCl(g) Express your
answer using four significant figures.
Calculate ΔH∘ for BaO(s)+CO2(g)→BaCO3(s) Express your answer
using four significant figures.
Calculate ΔG∘ for BaO(s)+CO2(g)→BaCO3(s) Express your answer
using four significant figures.