Dimethylhydrazine is a carbon-hydrogen-nitrogen compound used in
rocket fuels. When burned completely, a 0.312 g sample...
Dimethylhydrazine is a carbon-hydrogen-nitrogen compound used in
rocket fuels. When burned completely, a 0.312 g sample yields 0.458
g CO2 and 0.374 g H2O. What is the empirical formula of
diemthylhydrazine?
A 4.043 sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of dioxygen, producing 9.191 g CO2 and 3.762 g H2O. What percent by mass of oxygen is contained in the original sample? show your work and explain.
A 5.691 g sample of one such additive containing only lead,
carbon, and hydrogen was burned in an oxygen‑rich environment. The
products of the combustion were 6.194 g CO2(g) and 3.169 g H2O(g)
.Determine the empirical formula of the gasoline additive.
empirical formula:[ CHPb ]
a 0.580 g sample of a compound containing only carbon and
hydrogen contains .480 g of carbon and .100g of hydrogen. At STP
33.6mL of the gas has a mass of .087g. What is the molecular
formula for the compound? The answer should be C4H10. Please
explain with steps. Thank you.
A compound contains only carbon, hydrogen, nitrogen, and oxygen.
Combustion of 0.157g of the compound produced 0.213g CO2 and
0.0310g of H2O. In another experiment, 0.103g of the compound
produced 0.0230g of NH3. What is the emerical formula of the
compound? In a seperate experiment, the molar mass is found to be
454.3 g/mol. what is the molecular formula of the compound? hint:
assume that all carbon ends up in CO2 and all hydrogen ends up in
H2O.Also assume that...
Combustion analysis of a 0.2608 g sample of a compound
containing carbon, oxygen, and hydrogen only produced 0.5501 g of
carbon dioxide, and 0.2703 g of water.
Determine the empirical formula of this compound. If the molar
mass for this compound is 104.1 g/mole, find the molecular formula.
Write a complete balanced equation for the combustion reaction of
this compound.
When a 0.860 g sample of an organic compound containing C, H,
and O was burned completely in oxygen, 1.64 g of CO2 and
1.01 g of H2O were produced. What is the empirical
formula of the compound?
45. Upon combustion, a 0.8233 g sample of a compound containing
only carbon, hydrogen, and oxygen produced 2.445 g CO2 and 0.6003 g
H2O. Find the empirical formula of the compound.
PLEASE EXPLAIN VERY SINGLE STEP CLEARLY AS TO HOW YOU GOT
THERE
Combustion of a 0.9827-g sample of a compound containing only
carbon, hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of
H2O. What is the empirical formula of the compound?
Of the choices below, which would be the best for the lining of
a tank intended for use in storage of hydrochloric acid? Explain
your
reasoning.
(2)
A) copper
B) zinc
C) nickel
D) iron
E) tin
A compound contains only carbon, hydrogen, and oxygen.
Combustion of 54.05 g of the compound yields 79.22 g of
CO2 and 32.43 g of H2O.
The molar mass of the compound is 120.104 g/mol.
*Each part of this problem should be submitted separately to
avoid losing your work*
1. Calculate the grams of carbon (C) in 54.05 g of the
compound: grams
2. Calculate the grams of hydrogen (H) in 54.05 g of the
compound. grams
3. Calculate the grams of oxygen...
An organic compound contains carbon, hydrogen, and sulfur. A
sample of it with a mass of 2.712 g was burned in oxygen to give
gaseous CO2, H2O, and SO2. These
gases were passed through 311.2 mL of an acidified 0.0200
M KMnO4 solution, which caused the
SO2 to be oxidized to SO42-. Only
part of the available KMnO4 was reduced to
Mn2+. Next, 31.12 mL of 0.0300 M
SnCl2 was added to 31.12 mL portion of this solution,
which still...