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2 years ago

Oxides of nitrogen are pollutant gases which are emitted from car exhausts.

Chemistry

2 answers:

victus00 [196]2 years ago

5 0

Answer:

The correct answer is option B.

Explanation:

Mass of $N_xO_y$ ,m= 0.23 g

Molar mass of $N_xO_y=M=14 g\mol\times x+16 g/mol\times y$

$n=\frac{m}{M}$

Volume occupied by the $N_xO_y=120 cm^3=0.120 dm^3$

$1 cm^3 = 0.001 dm^3$

1 mol of gas molecules occupies 24.0 $dm^3$ .

Then n moles of $N_xO_y$ will occupy volume of $0.120 dm^3$ .

$n\times 24.0 dm^3/mol=0.120 dm^3$

n = 0.005 moles

$0.005 mol=\frac{0.23 g}{14g/mol\times x+16 g/mol\times y}$

$14x+16y=46$

Putting values from option A: x = 1, y = 1

14 × 1+16× 1 ≠ 46

Putting values from option B: x = 1, y = 2

14 × 1+16× 2 = 46 (The correct answer)

Putting values from option C: x = 2, y = 1

14 × 2+16× 1 ≠ 46

Putting values from option D: x = 2, y = 4

14 × 2+16× 4 ≠ 46

V125BC [204]2 years ago

4 0

Let's look at the molar weight of the answers:
NO is 30 g/mol
NO2 is 46
N2O is 44
N2O4 is 124

We have the grams of the product, so we need the moles in order to calculate the molar weight. We us PV=nRT for this, assuming standard temperature and pressure. 
You were given the liters (.120L)
Std pressure is 1 atmosphere
You're looking for n, the number of moles
Temp is 293.15 kelvin, thats standard 
And r is the gas constant in liters-atm per mol kelvin

(.120 liters)(1atm)=n(293.15K)(.08206)
Solving for n is .0049883835 mol

.23g divided by .0049883 mol is about 46g/mol. You're answer is B I think, NO2

I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!

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Barium oxalate is used as a colorant to produce the green color in fireworks. Imagine that you have been assigned to prepare bar

JulsSmile [24]

Answer:

2.1

Explanation:

Calculation of moles of $Ba(OH)_2.8H_2O$

Mass of copper = 5.3 g

Molar mass of copper = 315.46 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{5.3\ g}{315.46\ g/mol}$

Moles of $Ba(OH)_2.8H_2O$ = 0.0168 moles

According to the reaction,

$Ba(OH)_2.8H_2O + H_2C_2O_4.2H_2O\rightarrow BaC_2O_4 + 12 H_2O$

1 mole of $Ba(OH)_2.8H_2O$ react with 1 mole of $H_2C_2O_4.2H_2O$

0.0168 moles of $Ba(OH)_2.8H_2O$ react with 0.0168 moles of $H_2C_2O_4.2H_2O$

Moles of $H_2C_2O_4.2H_2O$ = 0.0168 moles

Molar mass of $H_2C_2O_4.2H_2O$ = 126.07 g/mol

Thus,

Mass = Moles * Molar mass = 0.0168 moles * 126.07 g/mol = 2.1 g

Answer - 2.1

5 0

2 years ago

Consider the following hypothetical reaction: 2 P + Q â†’ 2 R + S The following mechanism is proposed for this reaction: P + P Q

aleksandr82 [10.1K]

Answer: the answer is option (D). k[P]²[Q]

Explanation:

first of all, let us consider the reaction from the question;

2P + Q → 2R + S

and the reaction mechanism for the above reaction given thus,

P + P ⇄ T (fast)

Q + T → R + U (slow)

U → R + S (fast)

we would be applying the Rate law to determine the mechanism.

The mechanism above is a three step process where the slowest step seen is the rate determining step. From this, we can see that this slow step involves an intermediate T as reactant and is expressed in terms of a starting substance P.

It is important to understand that laws based on experiment do not allow for intermediate concentration.

The mechanism steps for the reactions in the question are given below when we add them by cancelling the intermediates on the opposite side of the equations then we get the overall reaction equation.

adding this steps gives a final overall reaction reaction.

2P + Q ------------˃ 2R + S

Thus the rate equation is given as

Rate (R) = K[P]²[Q]

cheers, i hope this helps

3 0

2 years ago

Explain why the spectrum produced by a 1-gram sample of element Z would have the same spectral lines at the same wavelengths as

TEA [102]

The reason why the spectrum produced by a 1 gram sample of element z would have the same spectral lines at the same wavelengths as the spectrum produced by a 2gram is because Mass does not determine the spectral lines

hope this helps

6 0

2 years ago

Read 2 more answers

Why did you blank with the 0.0020 M Fe(NO3)3 solution as opposed to just DI water? What does it do to your spectrum? What chemic

Vlad1618 [11]

Answer:

The cuvette was blank with the solution so that the spectrometer will only read the solute absorbance. This also ensures that the spectrometer will ignore other absorbance fluctuations that normally occur due to the chemical make-up of water. The spectrometer only considered the absorbance of $FeNCS^{2+}$ as indicated on the spectrum. The reaction between the $Fe^{3+}$ and the $SCN^{-}$ are both clear liquids that form the orange liquid product $FeNCS^{2+}$ which creates the absorbance spectrum. Because the color of the solution is orange, it reflects this and similar colors while absorbing blueish hues. We can find the absorption of only the $FeNCS^{2+}$ by pre-rinsing the cuvette with each solution we intend to measure before placing it in the spectrometer. Also, wipe each cuvette with a kimwipe to remove all fingerprints that could effect the data collection.