85.0g of barium metal are added to 275ml of 3.55M solution of hydrochloric acid, how many milliliters of hydrogen gas are collected at 18.5oC and 755.5mmHg in this single replacement reaction?

0.024 ml of hydrogen gas are collected at and 755.5mmHg in this single replacement reaction

Explanation:

To calculate the moles :

To calculate the number of moles for given molarity, we use the equation:

The balanced chemical reaction is:

According to stoichiometry :

2 moles of require = 1 mole of

Thus 0.976 moles of will require= of

Thus is the limiting reagent as it limits the formation of product and is the excess reagent.

As 2 moles of give = 2 moles of

Thus 0.976 moles of give =  of

According to ideal gas equation:

P = pressure of gas = 755.5 mmHg = 0.994 atm   (760 mm Hg = 1 atm )

V = Volume of gas in L = ?

n = number of moles = 0.976

R = gas constant =

T =temperature =

   (1L=1000ml)

Thus 0.024 ml of hydrogen gas are collected at and 755.5mmHg in this single replacement reaction

it's c. elements are placed in rows based on how may valencies electrons have.