Question

In a 13 L vessel initially following reaction occur
C(s) + S2(g) ==>CS,(g) by 12g C, 64 g S2,76
g CS2, at 1027°C temperature then total pressure
is -
(1) 200R
(2) 158 R
(3) 100 R
(4) 79 R​

Answer 1

Answer : The correct option is, (3) 100 R

Explanation :

Using ideal gas equation,

$PV=nRT\\\\PV=\frac{w}{M}RT\\\\P=\frac{w}{M}\frac{RT}{V}$

As per question the formula will be,

$P=[\frac{w_C+w_{S_2}+w_{CS_2}}{M_C+M_{S_2}+M_{CS_2}}]\times \frac{RT}{V}$

where,

P = total pressure = ?

R = gas constant

T = temperature = $1027^oC=273+1027=1300K$

V = volume = 13 L

$w_c$ = mass of C = 12 g

$w_{S_2}$ = mass of $S_2$ = 64 g

$w_{CS_2}$ = mass of $CS_2$ = 76 g

$M_c$ = molar mass of C = 12 g/mole

$M_{S_2}$ = molar mass of $S_2$ = 64 g/mole

$M_{CS_2}$ = molar mass of $CS_2$ = 76 g/mole

Now put all the given values in the above formula, we get:

$P=\frac{12g+64g+76g}{12g/mole+64g/mole+76g/mole}\times \frac{R\times 1300K}{13L}$

$P=100R$

Therefore, the total pressure is, 100 R

Answer 2

Answer:200R

Explanation: