The molecular formula is D. C_8H_20O_4Si.
<em>Step 1</em>.Calculate the <em>empirical formula
</em>
a) Calculate the moles of each element
Moles of C= 196.01 g C × (1 mol C/12.01 g C) = 16.325 mol C
Moles of H = 41.14 g H × (1 mol H/1.008 g H) = 40.813 mol H
Moles of O = 130.56 g O × (1 mol O/16.00 g O) = 8.1650 mol O
Moles of Si = 57.29 g Si × (1 mol Si/28.085 g Si) = 2.0399 mol Si
b) Calculate the molar ratio of each element
Divide each number by the smallest number of moles and round off to an integer
C:H:O:Si = 8.0027:20.008:4.0027:1 ≈ 8:20:4:1
c) Write the empirical formula
EF = C_8H_20O_4Si
<em>Step </em>2. Calculate the <em>molecular formula</em>
EF Mass = 208.33 u
MF mass = 208.329 u
MF = (EF)_n
n = MF Mass/EF Mass = 208.329 u/208.33 u = 1.0000 ≈ 1
MF = C_8H_20O_4Si
0.11 moles of the gas are present in the sample of dry gas.
Explanation:
Data given:
mass of the gas = 2.1025 grams
volume of the gas = 2.850 litres
temperature = 22 degrees (273.15+22) = 295.15 K
Pressure = 740 mm Hg or 0.973 atm
moles of the gas =?
R = 0.08206 atmL/Mole K
From the ideal gas law the number of moles can be calculated in the sample of dry gas. Number of moles will be determined by the pressure exerted, volume and temperature of the gas.
The formula:
PV = nRT
n = 
putting the values in the above equation:
n = 
= 0.11 moles
0.11 moles of the dry gas is present in the sample given.
It would have to be paints consists of pigments,solvents, and binders. Once the [paint has been applied and has dried, the pigments are still able to determine the matched samples.
Your answer is
Ca(OH)₂ + 2HNO₃ → Ca(NO₃)₂ + 2H₂O I hope it is at least :P
