Question

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Answer 1

Answer:

2. 0.6

Explanation

2NaOH+CO2→Na2CO3 +H2O

Molar ratio 2 :1

40 g NaOH=1 mole NaOH= 1/2mole CO2

(According to molar ratio)

Total mixture of (CO+CO

2 )=0.8 mole

→ 2CO+O2

→2CO2

shows us that the ratio of CO:CO2

is 1:1. Therefore, if mixture was completely oxidized then there would be 0.8 mole CO

2 in total.

→ Of 0.8 mole we have already used 0.5 mole

→ We have 08−0.5=0.3 mole CO2

1 mole CO2

→2 moles NaOH

∴ 0.3 moles CO²

→0.6 moles NaOH

Answer 2

Answer:

2) 0.6 is the correct option.

Explanation:

Hi Dear,

Let us know what is given first

Given :

0.8 mole of mixture of CO and CO₂ requires 40g of NaOH to convert to Na₂CO₃

To Find :

More moles of NaOH if all the mixture contains only 0.8 mole of CO₂ to convert to Na₂CO₃

Solution :

Let us first write the reaction of NaOH with CO₂.

$2NaOH + CO_2 \longrightarrow Na_2CO_3 + 2H_2O$

So, according to the reaction, we get that for 2 moles of NaOH and 1 mole of CO₂, we get 1 mole of Na₂CO₃

Given that, 40 gm of NaOH is used up for mixture of 0.8 moles of CO and CO₂. [Note that, CO doesn't react with NaOH]

We know that, molecular mass of NaOH is 40 gm

So, 1 mole of NaOH is used up in the given question

Hence, according to the reaction, we can find that if 1 mole of NaOH is reacted then CO₂ is reacted by 0.5 moles [2 : 1 = 1 : 0.5]

Therefore, we can conclude that we have 0.5 moles of CO₂ in the mixture and rest is CO

So, number of moles of CO = 0.8 - 0.5 = 0.3 moles

Thus, 0.3 moles of CO is available in the mixture

Now, we have to find if all this CO is CO₂ then what are the extra moles of NaOH required.

So, for 0.3 moles of CO₂, we need 0.6 moles of NaOH [NaOH : CO₂ = 2 : 1]

∴ 0.6 extra moles of NaOH is required to complete the reaction if all CO are CO₂

❖ Extra information :

$\text { \diamond Number of moles = \Large {\text { \frac{\textsf{Weight of the compound}}{\textsf {Molecular mass of the compound}} }}}$

Hope it  helps!!