Answer:
The new temperature is 34.21 °C
Explanation:
Step 1: Data given
Temperature of the system = 15°C
Pressure at 15°C is 1.50 atm
The pressure rose to 1216 torr (=1216/760 = 1.6 atm)
Step 2: Calculate the new temperature
P1/T1 = P2/T2
⇒ with P1 = the initial pressure = 1.50 atm
⇒ with T1 = the initial temperature = 15°C = 288.15 K
⇒ with P2 = the initial pressure = 1.60 atm
⇒ with T2 = the initial temperature = TO BE DETERMINED
T2 = T1 * (P2 / P1)
T2 = 288.15 * (1.60/1.50)
T2 = 307.36 K = 34.21 °C
The new temperature is 34.21 °C
The pressure increases as temperature increases, as a gas is heated it expands, so in a confined container (constant volume) pressure must increase, this can be observed through the universal gas law (pv=nRT)
Answer:
1455.6
Explanation: you first convert 2250ml to l by dividing by 1000 so you get 2.25l then you use Boyles law which is p1v1=p2v2 then insert values
35.75*100=p2*2.25 then divide both sides by 2.25 then you get 1455.6
