2 C4H10+13 O2 = 8 CO2+10 H2O identify the above chemical reaction type.

how many moles of water are produced when 43 grams of oxygen gas are reacted.

This chemical reaction is a combustion.

n = 1.8mol

Explanation:

The ratio of oxygen to water is 13 to 10

The ratio of oxygen to water is also 43 grams to x

Cross multiply: 13x = 430 grams

Isolate x: x = 33.0769g

Remember that n = mass/Molar mass

The molar mass of water is 18.01528 g/mol

n = 33.0769/18.01528

n = 1.836048

"the periodic table is arranged in order of atomic number."

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: