<u>Answer:</u>
<u>For 2:</u> The % yield of the product is 92.34 %
<u>For 3:</u> 12.208 L of carbon dioxide will be formed.
<u>Explanation:</u>
The percent yield of a reaction is calculated by using an equation:
......(1)
Given values:
Actual value of the product = 78.4 g
Theoretical value of the product = 84.9 g
Plugging values in equation 1:
Hence, the % yield of the product is 92.34 %
The number of moles is defined as the ratio of the mass of a substance to its molar mass.
The equation used is:
......(2)
Given mass of carbon dioxide = 24 g
Molar mass of carbon dioxide = 44 g/mol
Plugging values in equation 1:
<u>At STP conditions:</u>
1 mole of a gas occupies 22.4 L of volume
So, 0.545 moles of carbon dioxide will occupy = 
of volume
Hence, 12.208 L of carbon dioxide will be formed.
Answer:
a) rate law1 = k[NO2]²
b) rate law2 = k[NO][O3]
Explanation:
NO2(g) + CO(g) → NO(g) + CO2(g)
NO(g) + O3(g) → NO2(g) + O2(g)
When [NO2] in reaction 1 is doubled, the reaction quadruples
Rxn is second order.
rate law1= [NO2]^a [CO]^b
rate law1= [NO2]² [CO]^0
rate law1 = k[NO2]²
When [NO] in reaction 2 is doubled, the rate doubles.
Rxn is first order
The ratio is 1:1
this makes the rate law2 = k[NO][O3]
Options are as follow,
A) <span>Constant volume, no intermolecular forces of attraction,energy loss in collisions
B) </span><span>No volume, strong intermolecular forces of attraction, perfectly elastic collisions
C) </span><span>Constant volume, no intermolecular forces of attraction, energy gain during collisions
D) </span><span>No volume, no intermolecular forces of attraction, perfectly elastic collisions
Answer:
Option-D (</span>No volume, no intermolecular forces of attraction, perfectly elastic collisions) is the correct answer.
Explanation:
As we know there are no interactions between gas molecules due to which they lack shape and volume and occupies the shape and volume of container in which they are kept. So, we can skip Option-B.
Secondly we also know that the gas molecules move randomly. They collide with the walls of container causing pressure and collide with each other. And these collisions are perfectly elastic and no energy is lost or gained during collisions. Therefore Option-A and C are skipped.
Now we are left with only Option-D, In option D it is given that ideal gas has no volume. This is true related to Ideal gas as it is stated in ideal gas theories that molecules are far apart from each other and the actual volume of gas molecules compared to volume of container is negligible. Hence, for ideal gas Option-D is a correct answer.
