The volume of a gas is 27.5 ml at 22*C and 0.974 atm. What will be the volume if the temperature decreases to 15*C and the pressure increases to 0.993 atm?

26.33mL

Explanation:

In solving this question, we apply the general gas equation

(P1×V1)/T1 = (P2×V2)/T2

P1= initial pressure of the gas=0.974atm

V1= intial volume the gas occupies =27.5mL

T1=initial temperature of the gas =22°C =22+273K=295K

P2 = Final pressure of the gas = 0.993atm

V2= final volume of the gas = ?

T2 = final temperature of the gas = 15°C = 15+273=288K

From (P1×V1)/T1 = (P2×V2)/T2, we make V2 subject of formula

V2=(P1×V1×T2)/(P2×T2)

We substitute the given values

V2=(0.974×27.5×288)/(0.993×295)

V2=7714.08/292.935

V2=26.33mL

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:

1.solid

2.carbon dioxide

3.helium