Question

At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8655-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22

Answer #1

At elevated temperatures, solid sodium chlorate NaClO3
decomposes to produce sodium chloride, NaCl, and O2 gas. A 0.8948 g
sample of impure sodium chlorate was heated until the production of
oxygen ceased. The oxygen gas was collected over water and occupied
a volume of 63.2 mL at 23.0 C and 738 Torr. Calculate the mass
percentage of NaClO3 in the original sample. Assume that none of
the impurities produce oxygen on heating. The vapor pressure of
water is 21.07 Torr...

At elevated temperatures, solid sodium chlorate NaClO3decomposes
to produce sodium chloride, NaCl, and O2 gas. A 0.9560 g sample of
impure sodium chlorate was heated until the production of oxygen
ceased. The oxygen gas was collected over water and occupied a
volume of 63.6 mL at 23.0 ∘C and 737 Torr .
Calculate the mass percentage of NaClO3 in the original sample.
Assume that none of the impurities produce oxygen on heating. The
vapor pressure of water is 21.07 Torr...

A sample of soilid potassium chlorate was heated and decomposed
into solid potassium chloride and oxygen gas. The oxygen produced
was collected over water at 22 degrees celcius at a total pressure
of 745 Torr. the volume of the gas collected was 0.650 L, and the
vapor pressure of water at 22 degrees celcius is 21 torr.
2 KClO3(s)=2KCl(s)+3O2(g)
First calculate the partial pressre of oxygen in the gas
collected and determine the mass of potassium chlorate in the
sample...

Potassium chlorate (KClO3 molar mass 122.5 g/mol) decomposes
into oxygen gas and potassium chloride. When 3.25 grams of
potassium chlorate decomposes at 610 torr and 34*C, what is the
volume of oxygen gas produced? Remember to convert torr to atm and
Celcius to Kelvin. 2 KClO3 --> 3 O2(g) + 2 KCl (s).

When potassium chlorate is heated, potassium chloride and oxygen
gas are formed. The percent yield of the reaction is 83.2%. How
much potassium chlorate must be decomposed to produce 198.5 grams
of oxygen?

Part A
How much potassium chlorate is needed to produce 22.0
mL of oxygen gas at 675. mmHg and
22. ∘C?
Express the mass to three significant digits.
?g
Part B
If oxygen gas were collected over water at 22 ∘C and
the total pressure of the wet gas were 710 mmHg , what
would be the partial pressure of the oxygen?
Express the partial pressule in mm Hg to three significant
digits
?mmHg
Part C
An oxide of nitrogen was found by...

The compound Nd2(C2O4)3
decomposes when heated according to the equation below.
Nd2(C2O4)3(s)
➝ 2 Nd (s) + 6 CO2(g)
An impure sample of material contains a small amount of
Nd2(C2O4)3 . The sample
is heated and the gas produced collected by downward displacement
of water. A total of 166.5 ml of gas is collected at a temperature
of 22.0ºC when the atmospheric pressure is 680.0 torr.
[The vapor pressure of water at 22.0ºC is 19.83
torr.]
Calculate the number of...

A 2.00 g sample of HgO decomposes according to the reaction
below to yield oxygen gas, which is collected at 300 K and 0.910
atm. What volume of oxygen is collected?
2 HgO (s) → 2 Hg (l) + O2 (g)

A 0.4230 g sample of impure sodium nitrate (contains sodium
nitrate plus inert ingredients) was heated, converting all the
sodium nitrate to 0.1064 g of sodium nitrite and oxygen gas.
Determine the percent of sodium nitrate in the original sample.

A sample of oxygen gas was collected over water. The total
pressure was 735 torr, the volume was 555 mL, and the temperature
was 31.0ºC. What mass of oxygen was collected? The vapor pressure
of water at 31.0ºC is 33.7 torr.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 8 minutes ago

asked 9 minutes ago

asked 14 minutes ago

asked 35 minutes ago

asked 49 minutes ago

asked 59 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago