Question

40 ml of CO is exploded with 60 ml of O2 at
constant temperature and pressure. Final volume of the gases in ml will be
(1) 70
(2) 80
(3) 100
(4) 120​

Answer 1

Answer:

Volume of the gases will be 80mL.

Explanation:

Since, the reaction is 2CO + O2 -> 2CO2.

The coefficients are   2ml    1ml        2ml.

Given that the volume of CO is 40 ml and the O2 is 60ml so we get that the CO is the limiting reagent here so the CO2 formed will be 40ml.

So the remaining O2 will be the 60ml of the O2 from which the 1/2*40 ml will be exploded. So, the remaining O2 will be 60 - 20 = 40ml.

Hence the total volume will be 40 + 40 = 80ml.

Answer 2

Answer : The volume of gas is, 40 ml

Explanation :

The balanced chemical reaction will be,

First we have to calculate the limiting and excess reagent.

From the balanced chemical reaction we conclude that,

At constant temperature and pressure,

of gas react with 22.4 L of gas

So, 0.04 L of gas react with of gas

That means, the gas is a limiting reagent and gas is an excess reagent.

Now we have to calculate the moles volume of gas.

As, of gas react to give of gas

So, 0.04 L of gas react with 0.04 L of gas

The volume of gas = 0.04 L = 40 ml

Therefore, the volume of gas is, 40 ml

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