if an ideal gas has a pressure 2.47 atm, a temperature 86.78C and has a volume of 23.83L how many moles are in the sample

Use PV = nRT

To find the number of moles in the sample, we can use the ideal gas law equation:

PV = nRT

where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature of the gas (in Kelvin)

First, let's convert the given temperature from Celsius to Kelvin:

T(K) = T(C) + 273.15
T(K) = 86.78 + 273.15
T(K) = 359.93 K

Now, we can substitute the given values into the ideal gas law equation:

2.47 atm * 23.83 L = n * (0.0821 L·atm/(mol·K)) * 359.93 K

Simplifying the equation:

58.9301 = n * 29.5789133

Dividing both sides by 29.5789133:

n = 58.9301 / 29.5789133
n ≈ 1.99 moles

Therefore, there are approximately 1.99 moles in the sample.

To find the number of moles in a gas sample, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)

In order to use this equation, we need to convert the given temperature from Celsius to Kelvin. The conversion between Celsius and Kelvin is T(K) = T(°C) + 273.15.

Given:
Pressure (P) = 2.47 atm
Temperature in Celsius (T) = 86.78°C
Volume (V) = 23.83 L

First, we convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 86.78 + 273.15
T(K) = 359.93 K

Now we can rearrange the ideal gas law equation to solve for n (number of moles):

n = PV / RT

Substituting the given values:
n = (2.47 atm * 23.83 L) / (0.0821 L·atm/mol·K * 359.93 K)

Now we can calculate the number of moles n:

n ≈ 1.042 mol

Therefore, there are approximately 1.042 moles in the given gas sample.