Question

when dissolved in dilute sulphuric acid 0.275 gram of a metal evolved 11 9.7 ml of hydrogen at 20 degree Celsius and 763 mm pressure what is the equivalent mass of the metal

Answer 1

hey there is a answer
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Answer 2

Given:

• Mass of metal (w1) = 0.275 grams
• Volume of Hydrogen Gas evolved = 119.7 mL
• Temperature (T1) = 20 degree Celsius
• Pressure (P1) = 763 mm Hg

To Find:

• Equivalent Mass of Metal

Solution:

First we will convert the given temperature T1 in Kelvin.

T1 = 20 Degree Celsius or 20 + 273 K = 293 K

We know that,

$\dfrac{P1 \times V1}{T1}  = \dfrac{P2 \times V2}{T2}$

Here:

P1 = 763 mm                           P2 = 760 mm

T1 = 293 K                              T2 = 273 K

V1 = 119.7 mL                          V2 = ?

To calculate V2 , we will use the above formula to derive a new formula.

V2 = $\dfrac{P1 \times V1 \times T2}{P2 \times T1}$

Substituting the values of P1, V1 , T1, P2 and T2 in the above equation, we get:

V2 = $\dfrac{763 \times 119.7 \times 273}{760 \times 293}$

V2 = 111.97 mL

Since, 22400 mL of H2 gas occupies 2g at STP

1 mL will occupy $\dfrac{2}{22400}$ g at STP.

Therefore, 111.97 mL will occupy = $\dfrac{2}{22400} \times 111.97$ g at STP

So, 119.7 mL H2 gas will have mass = 0.00997 g at STP.

We know that,

Equivalent Weight = $\sf \dfrac{Mass of metal taken}{Mass of H2 gas taken}$

Equivalent Weight of Metal = $\dfrac{0.275}{0.00997}$

Equivalent Weight of Metal = 27.5

Therefore, the equivalent weight of Metal is 27.5.