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raketka [301]
3 years ago
14

Consider two gases, A and B, are in a container at room temperature. What effect will the following changes have on the rate of

the reaction between these gases? The temperature is decreased at a constant volume.
Chemistry
2 answers:
Tatiana [17]3 years ago
8 0

Explanation:

As it is given that two gases A and B are mixed together and kept in a container with constant volume.

Also, kinetic energy of molecules is directly related to temperature as follows.

                K.E = \frac{3}{2}kT

As kinetic energy is directly proportional to temperature. So, when there will be decrease in temperature then kinetic energy of molecules will also decrease leading to less number of collisions between the molecules.

Hence, there will be decrease in rate of reaction.

Thus, we can conclude that when temperature is decreased at a constant volume then rate of reaction will also decrease.

Anna [14]3 years ago
4 0

The effect that the following changes have on the rate of the reaction between the gases A and B in a container when the temperature is decreased at a constant volume will decrease because the molecules of A and B are ineracting very slowly due to the decrease in temperature which results to the decrease in kinetic energy.

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At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L . What volume wo
Nostrana [21]

Taking into account the Charles's law, the same amount of gas at the same pressure and 65 ∘C would occupy a volume of 27.73 L.

<h3>Charles's Law</h3>

Charles's Law consists of the relationship that exists between the volume and the temperature of a certain quantity of ideal gas, at a constant pressure.

Volume is directly proportional to the temperature of the gas: if the temperature increases, the volume of the gas increases, while if the temperature of the gas decreases, the volume decreases.

Mathematically, Charles's law is a law that says that the quotient that exists between the volume and the temperature will always have the same value:

V÷ T= k

Considering an initial state 1 and a final state 2, it is satisfied:

V1÷ T1= V2÷ T2

<h3>Volume at 65°C</h3>

In this case, you know:

  • V1= 22.4 L
  • T1= 0 C= 273 K
  • V2= ?
  • T2= 65 C= 338 K

Replacing in Charles's law:

22.4 L÷ 273 K= V2÷ 338 K

Solving:

(22.4 L÷ 273 K) ×338 K= V2

<u><em>V2= 27.73 L</em></u>

Finally, the same amount of gas at the same pressure and 65 ∘C would occupy a volume of 27.73 L.

Learn more about Charles's law:

brainly.com/question/4147359

#SPJ1

3 0
1 year ago
20.00 mL of a 0.077 M solution of silver nitrate, AgNO3
melomori [17]
N= m/v n=0.077/.200 = 0.385
8 0
3 years ago
Why is the answer C for this problem?
pshichka [43]

Answer:

\boxed{\text{(C) X}$_{3}$P$_{2}}

Explanation:

Step 1. Identify the Group that contains X

We look at the consecutive ionization energies and hunt for a big jump between them

\begin{array}{crc}n & IE_{n} & IE_{n} - IE_{n-1}\\1 & 730 & \\2 & 1450 & 720\\3 & 7700 & 6250\\4 & 10500 & 2800\\\end{array}

We see a big jump between n = 2 and n = 3. This indicates that X has two valence electrons.

We can easily remove two electrons, but the third electron requires much more energy. That electron must be in the stable, filled, inner core.

So, X is in Group 2 and P is in Group 15.

Step 2. Identify the Compound

X can lose two valence electrons to reach a stable octet, and P can do the same by gaining three electrons.

We must have 3 X atoms for every 2 P atoms.

The formula of the compound is \boxed{\text{X}$_{3}$P$_{2}}$}.

4 0
3 years ago
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