I havent been at school for 8 days due to somthing wrong with my heart, but the teachers gave me work. I have no clue how to do them. I really need help please, There all due tomarrow.
The air in a dry, sealed 2L soda bottle has a pressure of 0.998 atm at sea level at a temperature of 34C. what will be it's pressure, if it is brought to higher altitude where the temperature is only 23C?
(P1V1)/T1 = (P2V2)/T2.
To solve this problem, you need to apply the ideal gas law, which relates the pressure, volume, and temperature of a gas.
The ideal gas law is expressed as:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles of the gas
R = ideal gas constant
T = temperature
To solve your specific problem, you need to find the new pressure when the temperature changes from 34C to 23C.
Step 1: Convert the temperatures to Kelvin.
To convert from Celsius to Kelvin, you need to add 273.15.
Initial temperature (T1) = 34C + 273.15 = 307.15 K
Final temperature (T2) = 23C + 273.15 = 296.15 K
Step 2: Use the ideal gas law formula to solve for the new pressure.
We can rearrange the ideal gas law equation to find the new pressure (P2) when the temperature changes. The equation becomes:
P1/T1 = P2/T2
Substituting the known values:
0.998 atm / 307.15 K = P2 / 296.15 K
Step 3: Solve for the new pressure (P2).
First, multiply both sides of the equation by 296.15 K:
0.998 atm * 296.15 K = P2 * 307.15 K
Then, divide both sides of the equation by 307.15 K:
(0.998 atm * 296.15 K) / 307.15 K = P2
Now, calculate this expression to find the new pressure (P2).
By performing the calculations, the new pressure when the temperature changes to 23C will be approximately 0.961 atm.