How many liters of hydrogen gas is formed from the complete reaction of 15.9 g c? assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 k ?

Answer : The volume of hydrogen gas formed is, 39.2 liters.

Explanation :

The balanced chemical reaction is:

First we have to calculate the moles of carbon (C).

Molar mass of carbon = 12 g/mole

Mass of carbon = 15.9 g

Now we have to calculate the moles of gas.

From the reaction we conclude that,

As, 1 mole of carbon reaction to give 1 mole of hydrogen gas

So, 1.325 mole of carbon reaction to give 1.325 mole of hydrogen gas

Now we have to calculate the volume of hydrogen gas by using ideal gas equation.

where,

P = Pressure of gas = 1.0 atm

V = Volume of gas = ?

n = number of moles   = 1.325 mole

R = Gas constant =

T = Temperature of gas = 360 K

Putting values in above equation, we get:

Therefore, the volume of hydrogen gas formed is, 39.2 liters.

possibly, yes.

explanation:

the amount of sugar you take in is dangerously high, risk of heart disease, high risk of diabetes, and etc.

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.