Apellet of zn of mass 10.0g is dropped into a flaskcontaining
dilute h2so4 at a pressure of p=1.00 bar and
temperature of 298k. what is the reaction thatoccures? calculate w
for the process.

Work done for the process is -390 J

Explanation:

The chemical equation for the reaction of zinc metal with sulfuric acid follows:

To calculate the number of moles, we use the equation:

Given mass of zinc = 10.0 g

Molar mass of zinc = 65.38 g/mol

Putting values in above equation, we get:

The equation given by ideal gas follows:

where, P = pressure of the gas

= Change in volume of the gas

T = Temperature of the gas = 298 K

R = Gas constant = 8.314 J/mol.K

n = number of moles of gas = 0.153 mol

Putting values in above equation, we get:

To calculate the work done, we use the equation:

Hence, work done for the process is -390 J

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.