Question

If 263 ml of a gas is collected at 47°c and 2.77 atm, what will the final temp be in C if the volume decreases to 195 mL and the pressure increases to 3.87 atm?

im stoopid so yeh pls help

Answer 1

`58.48^(\circ)\text{C}`

Step-by-step explanation:

`P_1` = Initial pressure = 2.77 atm

`V_1` = Initial volume = 263 mL

`T_1` = Initial temperature =
`47^(\circ)\text{C}=(47+273.15)\ \text{K}`

`P_2` = Final pressure = 3.87 atm

`V_2` = Final volume = 197 mL

`T_2` = Final temperature

We have the relation

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)\\\Rightarrow T_2=(P_2V_2)/(P_1V_1)* T_1\\\Rightarrow T_2=(3.87* 195)/(2.77* 263)* (47+273.15)\\\Rightarrow T_2=331.63\ \text{K}=331.63-273.15\\\Rightarrow T_2=58.48^(\circ)\text{C}`

The final temperature will be
`58.48^(\circ)\text{C}`.