At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20∘C to 25∘C

1 answer:

5 0

Answer: 0.0007 moles of $CO_2$ are released when the temperature rises.

Explanation:

To determine the moles, we utilize the ideal gas law, as follows:

$PV=nRT$

where,

P = gas pressure = 1.01 bar

V = gas volume = 1L

R = gas constant = $0.08314\text{ L bar }mol^{-1}K^{-1}$

The gas temperature = 20° C = (273 + 20)K = 293K

Substituting values into the equation gives:

$1.01bar\times 1L=n_1\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 293K\\n_1=0.04146moles$

The gas temperature = 25° C = (273 + 25)K = 298K

Substituting values into the equation gives:

$1.01bar\times 1L=n_2\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 298K\\n_2=0.04076moles$

Therefore, 0.0007 moles of $CO_2$ are released when the temperature increases from 20° C to 25° C.

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alisha [2963]

Answer:

During this process, energy is released as a bond is formed.

Explanation:

The elements present on the left side of the reaction equation are known as reactants, while those on the right are called the products.

In this case, N(g) and N(g) are the reactants, and N2(g) along with energy are the products.

Post-reaction, N(g) has vanished and has been replaced by N2(g). It confirms that a bond exists between the two N(g).

Moreover, energy has been released as part of the products (indicated on the right side)

The accurate statement is ''A bond is formed and energy is released''

5 0

3 months ago