1. mass of flask + cap = 92.53 g
2. mass of flask + cap + condensate = 94.34 g
3. mass of condensate = 1.81 g
4. volume of flask = 160 ml
5. temperature of water = 99.3 celsius
6. barametric pressure = 757 ml of mercury
7.. molar mass of gas(experimental) = ???
8. formula of gas = C2H5OH
9. molar mass based on formula = ??
10. percent error (#7-#9/100)/ #9 = ????
formula:
PV = nRt where n = moles = grams/Mm
n : PV = gRT/ Mm
Mm: Mm = gRT/PV
Something is wrong but I don't know what it is. The numbers go in this way.
M = gRT/PV where P=757/760 = 0.996
M = 1.81*0.08206*(273.2+99.3)/0.996*0.160 but if the answer is supposed to be the molar mass of C2H5OH it isn't even close.
To find the molar mass of the gas experimentally (#7), you can use the ideal gas law equation PV = nRT. Rearranging the equation, you get:
n = PV / RT
Now, let's calculate the value of n:
P = 757 mmHg (convert to atm by dividing by 760)
V = 160 ml (convert to liters by dividing by 1000)
R = 0.0821 L·atm/(mol·K) (ideal gas constant)
T = 99.3 + 273.15 K (convert Celsius to Kelvin)
Plugging in the values:
n = (757/760) * (160/1000) / (0.0821) * (99.3 + 273.15)
Once you have calculated the value of n, you can proceed to finding the molar mass of the gas based on the formula (#9).
To find the molar mass (#9) based on the formula, C2H5OH, you need to calculate the sum of the atomic masses of all the elements in the formula. This formula consists of 2 carbon (C) atoms, 6 hydrogen (H) atoms, and 1 oxygen (O) atom.
The atomic masses are as follows:
C: 12.01 g/mol
H: 1.008 g/mol
O: 16.00 g/mol
Now, calculate the molar mass based on the formula:
Mm = (2 * 12.01) + (6 * 1.008) + (1 * 16.00)
Once you have calculated both the experimental molar mass (#7) and the molar mass based on the formula (#9), you can find the percent error (#10).
To calculate the percent error:
Percent Error = ((Experimental Molar Mass - Molar Mass based on the Formula) / Molar Mass based on the Formula) * 100
Substitute the values into the formula to find the percent error.