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

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.