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3 years ago

Which of the three gases will have the highest average kinetic energy at a given temperature

Chemistry

1 answer:

Alona [7]3 years ago

4 0

This is an incomplete question, here is a complete question.

Which of the three gases will have the highest average kinetic energy at a given temperature?

A) HBr

B) NO₂

C) C₂H₆

Answer : All three gases will have the same average kinetic energy at a given temperature.

Explanation :

The formula for average kinetic energy is:

$K.E=\frac{3}{2}kT$

where,

K.E = average kinetic energy

k = Boltzmann’s constant

T = temperature

As we know that, average kinetic energy depends only on the temperature.

As the temperature of the all three gases are same. So, the all three gases will have the same average kinetic energy.

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Nitrogen dioxide is produced by combustion in an automobile engine. For the following reaction, 0.377 moles of nitrogen monoxide

Contact [7]

Answer:

The amount of NO₂ that can be produced 8.533 g

Explanation:

According to question

2 NO(g) + O₂(g) → 2 NO₂(g)

Given

Moles of nitrogen monoxide = 0.377

Moles of oxygen = 0.278

$'For NO'=\frac{Mole}{Stoichiometry}=\frac{0.377}{2} =0.1855\\'For O_{2} '=\frac{0.278}{1}= 0.278\\$

Since 'NO' is the limiting reagent according to this ratio.

According to equation

2 moles NO reacts to form 2 moles NO₂

So, 0.1855 moles NO give = 0.1855 moles of NO₂

Mass of 1 mole NO₂ = 46 g/mole

Mass of 0.1855 moles = 46 x 0.1855 = 8.533 g

5 0

3 years ago

A student is studying a sample of carbon dioxide gas inside a small syringe. At constant temperature the syringe has a volume of

Soloha48 [4]

The new pressure inside the syringe will be 1.25 atm

At constant temperatures, the volume of a gas is inversely proportional to its pressure.

Thus: P1V1 = P2V2

In this case, P1 = 3.0 atm, V1 = 89.6 mL, V2 = 215 mL

P2 = P1V1/V2

= 3 x 89.6/215

= 1.25 atm

More on gas laws can be found here: brainly.com/question/1190311

4 0

2 years ago

Which of the following would not cause an increase in the pressure of a gaseous system in a container? A The container is made l

ludmilkaskok [199]

Answer:

The container is made larger

Explanation:

5 0

3 years ago

Read 2 more answers

Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE?A) This reaction will be

Alja [10]

Answer: A) This reaction will be spontaneous only at high temperatures

Explanation:

$\Delta G$ = +ve, reaction is non spontaneous

$\Delta G$ = -ve, reaction is spontaneous

$\Delta G$ = 0, reaction is in equilibrium

Using Gibbs Helmholtz equation:

$\Delta G=\Delta H-T\Delta S$

Given : $\Delta H=+ve$

$\Delta S=+ve$

$\Delta G=(+ve)-T(+ve)$

$\Delta G=(+ve)(-ve)$

Thus the value of $\Delta G$ is negative and spontaneous when temperature is high.

4 0

3 years ago

When 5.00 g of Al2S3 and 2.50 g of H2O are reacted according to the following reaction: Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H

Debora [2.8K]

Answer:

$Y=58.15\%$

Explanation:

Hello,

For the given chemical reaction:

$Al_2S_3(s) + 6 H_2O(l) \rightarrow 2 Al(OH)_3(s) + 3 H_2S(g)$

We first must identify the limiting reactant by computing the reacting moles of Al2S3:

$n_{Al_2S_3}=5.00gAl_2S_3*\frac{1molAl_2S_3}{150.158 gAl_2S_3} =0.0333molAl_2S_3$

Next, we compute the moles of Al2S3 that are consumed by 2.50 of H2O via the 1:6 mole ratio between them:

$n_{Al_2S_3}^{consumed}=2.50gH_2O*\frac{1molH_2O}{18gH_2O}*\frac{1molAl_2S_3}{6molH_2O}=0.0231mol Al_2S_3$

Thus, we notice that there are more available Al2S3 than consumed, for that reason it is in excess and water is the limiting, therefore, we can compute the theoretical yield of Al(OH)3 via the 2:1 molar ratio between it and Al2S3 with the limiting amount:

$m_{Al(OH)_3}=0.0231molAl_2S_3*\frac{2molAl(OH)_3}{1molAl_2S_3}*\frac{78gAl(OH)_3}{1molAl(OH)_3} =3.61gAl(OH)_3$

Finally, we compute the percent yield with the obtained 2.10 g:

$Y=\frac{2.10g}{3.61g} *100\%\\\\Y=58.15\%$

Best regards.

7 0

3 years ago