Question
In: Chemistry
Nitrogen gas reacts with oxygen gas to form dinitrogen tetroxide. N2 (g) + 2 O2 (g)...
Nitrogen gas reacts with oxygen gas to form dinitrogen tetroxide.
N2 (g) + 2 O2 (g) → N2O4 (g)
A 1.8 L reaction vessel, initially at 298 K, contains nitrogen gas at a partial pressure of 337 mmHg and oxygen gas at a partial pressure of 445 mmHg .
What is the pressure of N2O4 in the reaction vessel after the reaction?
Enter your answer numerically, in terms of mmHg.
Please show all work
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction...
Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in
dinitrogen pentoxide and has a half-life of 2.81 h at 25 ∘C.
If a 1.5-L reaction vessel initially contains 760 torr of N2O5
at 25 ∘C, what partial pressure of O2 is present in the vessel
after 225 minutes?
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction...
Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in
dinitrogen pentoxide and has a half-life of 2.81 h at 25 ∘C.
If a 1.7-L reaction vessel initially contains 760 torr of N2O5
at 25 ∘C, what partial pressure of O2 is present in the vessel
after 205 minutes?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia
gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g)
Part B
How many grams of NH3 can be produced from 2.15 mol of N2 and
excess H2.
Part C
How many grams of H2 are needed to produce 13.02 g of NH3?
Part D
How many molecules (not moles) of NH3 are produced from
4.83×10−4 g of H2?
Express your answer numerically as the number of molecules.
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia
gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3 How many
grams of H2 are needed to produce 10.70 g of NH3? How many
molecules (not moles) of NH3 are produced from 3.21×10−4 g of
H2?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia
gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3 How many
grams of H2 are needed to produce 10.70 g of NH3? How many
molecules (not moles) of NH3 are produced from 3.21×10−4 g of
H2?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia
gas, NH3, according to the equation
3H2(g)+N2(g)→2NH3(g)
1a. How many grams of NH3 can be produced from 2.60 mol of N2
and excess H2
1b. How many grams of H2 are needed to produce 11.32 g of
NH3?
1c. How many molecules (not moles) of NH3 are produced from
4.06×10−4 g of H2?
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia
gas, NH3, according to the equation
3H2(g)+N2(g)→2NH3(g)
a. How many grams of H2 are needed to produce 11.70 g of
NH3?
b. How many molecules (not moles) of NH3 are produced from
4.42×10−4 g of H2?
Hydrazine (N2H4) reacts with oxygen gas to form nitrogen gas and water. A. Write a balanced...
Hydrazine (N2H4) reacts with oxygen gas to form nitrogen gas and
water.
A. Write a balanced equation for this reaction
B.How many grams of water are theoretically produced when 15.8g
of hydrazine react with 18.3 g. of oxygen?
C.How many grams of the excess reactant remain?
D.9.16 g of water are actually produced. What is the percent
yield for this reaction?
E. Using the percent yield from (d) how many kilograms of water
can actually be produced from 292 L...
Hydrazine, N 2 H 4 , reacts with oxygen to form nitrogen gas and water. N...
Hydrazine, N 2 H 4 , reacts with oxygen to form nitrogen gas and
water. N 2 H 4 ( aq ) + O 2 ( g ) ⟶ N 2 ( g ) + 2 H 2 O ( l ) If
2.45 g of N 2 H 4 reacts with excess oxygen and produces 0.650 L of
N 2 , at 295 K and 1.00 atm, what is the percent yield of the
reaction?
Hydrazine, N2H4, may react with oxygen to form nitrogen gas and water. N2H4(aq) + O2(g) ->...
Hydrazine, N2H4, may react with oxygen to form nitrogen gas and
water. N2H4(aq) + O2(g) -> N2(g) + 2H2O(l) If 3.65 g of N2H4
reacts and produces 0.950 L of N2, at 295 K and 1.00 atm, what is
the percent yield of the reaction?
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