2 g (an excess) of iron is added to 50 cm of 0.5 M sulfuric acid. When the reaction is over,
the reaction mixture is filtered. The mass of the
unreacted iron is found to be 0.6 g. (A,: Fe = 56.)
a What mass of iron took part in the reaction?
b How many moles of iron atoms took part?
c How many moles of sulfuric acid reacted?
d Write the equation for the reaction, and deduce
the charge on the iron ion that formed.
e What volume of hydrogen (calculated at rtp)
bubbled off during the reaction?

a patient chooses to not take a beneficial medical treatment.

explanation:

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:

2b2t

explanation:

2b2t