A sample of gas of unknown pressure occupies 0.766 L at a temperature of 298 K. The same sample of gas is then tested under known conditions and has a pressure of 32.6 kPa and occupies 0.644 L at 303 K. What was the original pressure of the gas

26.96 kPa

Explanation:

Applying,

PV/T = P'V'/T' Equation 1

Where P = Initial pressure, V = Initial volume, T = Initial temperature, P' = Final pressure, V' = Final volume, T' = Final temperature.

make P the subject of the equation

P = P'V'T/VT' Equation 2

From the question,

Given: V = 0.766 L, T = 298 K, P' = 32.6 kPa, V' = 0.644 L, T' = 303 K

Substitute these values into equation 2

P = (32.6×0.644×298)/(0.766×303)

P = 26.96 kPa

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:

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