A0.435 g sample of a metal, m, reacts completely with sulfuric acid according to m ( s ) + h 2 so 4 ( aq ) ⟶ mso 4 ( aq ) + h 2 ( g ) a volume of 201 ml of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. atmospheric pressure is 756.0 torr, and the temperature is 25 °c. calculate the molar mass of the metal.

The molar mass of metal is 52.4 g/mol

Explanation:

To calculate the moles of hydrogen gas collected, we use the equation given by ideal gas which follows:

where,

P = pressure of the hydrogen gas = Total pressure - vapor pressure of water = (756.0 - 23.8 ) torr = 732.2 torr  

V = Volume of the gas = 201 mL = 0.201 L    (Conversion factor:  1 L = 1000 mL)

T = Temperature of the gas =

R = Gas constant =

n = number of moles of hydrogen gas = ?

Putting values in above equation, we get:

The given chemical equation follows:

By Stoichiometry of the reaction:

1 mole of hydrogen gas is formed by 1 mole of metal

So, 0.0083 moles of hydrogen gas will be formed by = of metal

To calculate the molar mass of metal from given number of moles, we use the equation:

Moles of metal = 0.0083 moles

Given mass of metal = 0.435 g

Putting values in above equation, we get:

Hence, the molar mass of metal is 52.4 g/mol

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explanation:

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i'm pretty sure its b i might be wrong though!