1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Lady bird [3.3K]
3 years ago
11

The emission of NO₂ by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea r

educes NO (which oxidizes in air to form NO₂) according to the following reaction: 2CO(NH₂)₂(g)+4NO(g)+O₂(g)→4N₂(g)+2CO₂(g)+4H₂O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.37 L/s at 657 K and contains a partial pressure of NO of 14.0 torr .What total mass of urea is necessary to react completely with the NO formed during 8.1 hours of driving?Express answer in g.
Chemistry
1 answer:
liq [111]3 years ago
4 0

Answer:

There is 709.1 grams of urea needed.

Explanation:

<u>Step 1:</u> The balanced equation:

2CO(NH2)2(g)+4NO(g)+O2(g)→4N2(g)+2CO2(g)+4H2O(g)

<u>Step 2:</u> Data given

The exhaust stream of an automobile has a flow rate of 2.37 L/s

This happens at a temperature of 657 Kelvin

The partial pressure of NO is 14.0 torr

<u>Step 3:</u> Calculating the volume during 8.1 hours

V = 2.37L/s ∙ 8.1hr ∙3600s/hr = 69109.2L = 69.1092m³

<u>Step 4</u>: Calculate  the partial pressure of nitric oxide:

p = 14 torr ∙ 101325Pa/760torr = 1866.5Pa

<u>Step 5:</u> Calculating number of moles of NO

⇒ We use the ideal gas law P*V=n*R*T

n(NO) = P*V/R*T

with P= The partial pressure of NO = 1866.5 Pa

with V =the volume of NO = 69.1092m³

with R = the gas constant = 8.314472 Pa*m³/mol*K

with T = 657 Kelvin

n(NO) = 1866.5Pa ∙ 69.1092m³ / (8.314472Pa*m³/mol*K ∙ 657K)

= 23.61 mol es

<u>Step 6:</u> Calculate moles of urea

Since there is consumed 2 moles of urea per 4 moles of nitric oxide.

This means for 24.432 moles of NO, there is consumed 23.61 /2 = 11.806 moles of urea.

<u>Step 7</u>: Calculate mass of urea

m(CO(NH₂)₂) = 11.806 moles ∙ 60.06g/moles = 709.07g

There is 709.1 grams of urea needed.

You might be interested in
What does the peak of a probability curve for an electron in an atom indicate?
Eduardwww [97]
The distance from the nucleus at which the electron is most likely to be found
3 0
3 years ago
Read 2 more answers
Write Qc for each of the following:(1) Gaseous sulfur tetrafluoride reacts with liquid water to produce gaseous sulfur dioxide a
snow_tiger [21]

Answer : The expression for reaction quotient will be :

(1) Q_c=\frac{[SO_2][HF]^4}{[SF_4]}

(2) Q_c=\frac{[O_2]^2[Xe]}{[XeF_2]}

Explanation :

Reaction quotient (Q_c) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

(1) The given balanced chemical reaction is,

SF_4(g)+2H_2O(l)\rightarrow SO_2(g)+4HF(g)

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.  So, the expression for reaction quotient will be :

Q_c=\frac{[SO_2][HF]^4}{[SF_4]}

(2) The given balanced chemical reaction is,

2MoO_2(s)+XeF_2(g)\rightarrow 2MoF(l)+Xe(g)+2O_2(g)[/texIn this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.  So, the expression for reaction quotient will be :[tex]Q_c=\frac{[O_2]^2[Xe]}{[XeF_2]}

7 0
3 years ago
This is my chemistry worksheet. It's a new topic my teacher will barely review with us. Help please???
TEA [102]
So to balance an equation, you need to get the same amount of each type of element on either side of the --> . So you pretty much are given the subscripts in the equations and you need to add coefficients (just normal numbers) in front of any formula that needs it, keeping anything balance.
KCl_{3}  + O_{2}  -\ \textgreater \  KCl_{3}
turns into
2KCl_{3}+ 3O_{2} -> 2KCl_{3}

These coefficient numbers are the molar ratios, so 2 moles of KCl3 for every 3 moles of O2   so 1. 3:2

Then you can use these ratios of find out how many moles of one thing are needed if you are given the amount of another.
\frac{moles of element 1}{cofficient 1}  =  \frac{moles of element 2}{cofficient 2}
and use cross multiplication to solve for whatever you don't know


<span />
6 0
3 years ago
This <br> Question please
Marizza181 [45]

Answer:

See detailed explanation.

Explanation:

Hello!

i. In this case, since the given chemical reaction is exothermic due to the negative change in the enthalpy of reaction, we infer that according to the mentioned principle, by lowering the temperature the reaction will shift rightwards and therefore the yield is increased; thus, you need a lower temperature than the specified.

ii. In this case, since the reaction has less moles at the products side, according to the mentioned principle it'd be necessary to rise the pressure in order to increase the yield, since the increase of pressure favors the reaction side with the fewest number of moles.

Best regards!

4 0
2 years ago
A similar reaction is used frequently in laboratory experiments as an indicator. Can you guess what that might be?
svp [43]

Answer: ph scale

Explanation:

7 0
2 years ago
Other questions:
  • The molar percent of a in stream 3 is _________ mol% a in stream 1.
    14·1 answer
  • LaShawna and her family went to Yellowstone National Park. They saw a spring called Green Dragon Spring. Steam was rising off th
    13·2 answers
  • The equation for the reaction is
    14·1 answer
  • The muscle in Lane's arm would best be described as -
    9·1 answer
  • The prefix centi- means
    11·2 answers
  • Calculate the theoretical yield of aspirin obtained when 2.0 g of salicylic acid and 5.0 mL of acetic anhydride (density = 1.08
    14·1 answer
  • Help me out? thank you.
    5·2 answers
  • NEED HELP FAST! 20 POINTS!!
    15·2 answers
  • What is co-wolent bond?<br><br>​
    15·1 answer
  • 4.What volume of hydrogen gas at STP is produced when 2.5 grams of zinc react with an
    10·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!