A gas in a rigid container at 25°C has a pressure of 0.96 atm. A change in temperature causes the pressure to increase to 1.25 atm. What is the new temperature of the gas? Use StartFraction P subscript 1 over T subscript 1 EndFraction equals StartFraction P subscript 2 over T subscript 2 EndFraction.. –44.2°C 32.6°C 115°C 388°C

Answer is c115°C

Explanation:

Gay-Lussacs law says that pressure of a gas is the same as temperature when the volume is kept the same

P / T = k

where P - pressure , T - temperature in kelvin and k - constant

parameters for the first time are on the left side of the equation and parameters for the second instance are on the right side of the equation

T1 - 25 °C + 273 = 298 K

substiuting the values in the equation

T2 = 388 K

temperature in celcius - 388 K - 273 = 115 °C

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: