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Under certain conditions, water can be separated into oxygen and hydrogen gases according to the equation 2H20 →
2H2 + O2
In a lab, 112g of hydrogen gas and 888g of oxygen gas were collected. Student A says that the amount of water to start
cannot be determined, but Student B says that the water must have been 1000g. Who is correct?
(1 point)

Respuesta :

Oseni

The approximate amount of water used in the reaction is 1000 g. Student B is correct.

From the equation of the reaction, the mole ratio of the H2 produced and the H2O separated is 1:1.

mole of H2 produced = mass/molar mass

                                        = 112/2

                                           = 56 moles

This means that 56 moles of H2O was also separated.

Mass of 56 moles of H2O = 56 x 18

                                           = 1,008 g

Also from the equation of the reaction, the mole ratio of O2 produced to water separated is 1:2.

Mole of O2 produced = 888/32

                                       = 27.75 moles

Equivalent mole of H2O = 27.75 x 2

                                        = 55.5 moles

Mass of 55.5 moles of H2O = 55.5 x 18

                                               = 999 g

Thus, the approximate amount of water used in the reaction must have been 1000 g. Student B is correct.

More on law of conservation of matter can be found here:https://brainly.com/question/9434062?referrer=searchResults