A chemist determined by measurements that 0.030 moles of barium participated in a chemical reaction. Calculate the mass of barium that participated in the chemical reaction. Round your answer to 2 significant digits.

4.1 g of barium precipitated.

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number of particles.

To calculate the moles, we use the equation:

Given : moles of barium = 0.030

Molar mass of barium = 137 g/mol

x= 4.1 g

Thus there are 4.1 g of barium that precipitated.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: