please I and my friend has been trying this one.
If there there are 2.7*10^19 molecules are there in 1.0cm3 of a gas at 273k and pressure 1.0*10 ^5Pa. How many molecules are there in 1.0cm3 of the gas at 350k and pressure 1.0*10 ^5Pa.
All you did was heat it up?
P V= n R T
so
n/V = density = P/RT
You tell me that P and V constant and so is R
so
n= k/T or (nT) = constant
so
2.7*10^19 * 273 = n * 350
n = 2.7 * (273/350) * 10^19
tanks bro
To solve this problem, we can use the ideal gas law equation, which relates the number of molecules (n) of a gas to the pressure (P), volume (V), and temperature (T):
PV = nRT
Where:
P is the pressure in Pascals (Pa)
V is the volume in cubic meters (m^3)
n is the number of molecules
R is the ideal gas constant, approximately 8.314 J/(mol·K)
T is the temperature in Kelvin (K)
Let's begin by finding the value of n for the first scenario, at 273K and 1.0*10^5 Pa.
Given:
Volume (V1) = 1.0 cm^3 = 1.0 * 10^-6 m^3
Temperature (T1) = 273 K
Pressure (P1) = 1.0 * 10^5 Pa
Now we can rearrange the ideal gas law equation to solve for n:
n = PV / RT
Substituting the given values:
n1 = (P1 * V1) / (R * T1)
Calculating n1:
n1 = (1.0 * 10^5 Pa * 1.0 * 10^-6 m^3) / (8.314 J/(mol·K) * 273 K)
Now, let's calculate the value of n2 for the second scenario, at 350K and 1.0 * 10^5 Pa.
Given:
Temperature (T2) = 350 K
Pressure (P2) = 1.0 * 10^5 Pa
Using the same formula:
n2 = (P2 * V1) / (R * T2)
Substituting the given values:
n2 = (1.0 * 10^5 Pa * 1.0 * 10^-6 m^3) / (8.314 J/(mol·K) * 350 K)
Now you can calculate n1 and n2 using the given formulas and values.