The volume of oxygen required to burn completely 90 dm $^{3}$ of butane under similar conditions of temperature and pressure is ______.

$2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O$

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Solution

The ratio $= 2 : 13 : 8 : 10$ .
If 2 $d m^{3}$ of butane burn completely in presence of 13 $d m^{3}$ of oxygen.
Then, 90 $d m^{3}$ of butane burn completely in presence of
= $\frac{90}{2} \times 13$ = 585 $d m^{3}$ .
Thus, 585 $d m^{3}$ of oxygen is required.

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Q. What volume of oxygen is required to burn completely

90 d m^{3}

of butane under similar conditions of temperature and pressure?

2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O

Q. Find the amount of oxygen required for the complete combustion of 4 mol of butane.

2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O

Q. Find the amount of oxygen required for the complete combustion of 4 mol of butane.

2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O

(a) (i) What volume of oxygen is required to burn completely $90 d m^{3}$ of butane under similar conditions of temperature and pressure?

$2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O$

(ii) the vapour density of a gas is 8. What would be the volume occupied by 24.0 g of the gas at STP?
(iii) A vessel contains X number of molecules of hydrogen gas at a certain temperature and pressure. How many molecules of nitrogen gas would be present in the same vessel under the same conditions of temperature and pressure?

(b) $O_{2}$ is evolved by heating $K C l O_{3}$ using $M n O_{2}$ as a catalyst.

$2 K C l O_{3} M n O_{2} - --- \to 2 K C l + 3 O_{2}$

(i) Calculate the mass of $K C l O_{3}$ required to produce 6.72 litres of $O_{2}$ at STP.
[atomic masses of $K = 39, C l = 35.5, O = 16]$
(ii) Calculate the number of moles of oxygen present in the above volume and also the number of molecules.
(iii) Calculate the volume occupied by 0.01 mole of $C o_{2}$ at STP.

Q. Butane gas burns in air according to the following reaction,

2 C_{4} H_{10} + 13 O_{2} ⟶ 10 H_{2} O + 8 {C O}_{2}

Suppose the initial and final temperatures are equal and high enough so that all reactants and products act as perfect gases. Two moles of butane are mixed with

13

moles of oxygen and then completely reached. Find the final pressure (if the volume remains unchanged and the pressure before the reaction is

P_{0}

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The volume of oxygen required to burn completely 90 dm3 of butane under similar conditions of temperature and pressure is ______.2C4H10+13O2→8CO2+10H2O

The ratio =2:13:8:10.If 2 dm3 of butane burn completely in presence of 13 dm3 of oxygen.Then, 90 dm3 of butane burn completely in presence of= 902×13 = 585 dm3.Thus, 585 dm3 of oxygen is required.

The volume of oxygen required to burn completely 90 dm $^{3}$ of butane under similar conditions of temperature and pressure is ______.

$2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O$

The ratio $= 2 : 13 : 8 : 10$ .
If 2 $d m^{3}$ of butane burn completely in presence of 13 $d m^{3}$ of oxygen.
Then, 90 $d m^{3}$ of butane burn completely in presence of
= $\frac{90}{2} \times 13$ = 585 $d m^{3}$ .
Thus, 585 $d m^{3}$ of oxygen is required.