Let 4 moles of methanol (liquid) combust in 3 moles of gaseous oxygen to form gaseous carbon dioxide and water vapor. suppose this occurs in a chamber of fixed volume and fixed temperature. if the original pressure is 1.0 atm, what is the final pressure in the chamber. express your answer in atm. enter a numerical value, do not enter units. assume liquids take up negligible volume.

The final pressure is 2.0 atm

Explanation:

Step 1: Data given

Number of moles methanol = 4 mol

Number of moles oxygen = 3 mol

original pressure is 1.0 atm

Step 2: The balanced equation

2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l)

Step 3: Calculate final pressure

For 2 moles of methanol consumed, we need 3 moles O2 to produce 2 moles CO2 and 4 moles H2O

We started with 3 moles of O2 gas.  

Since methanol is not a gas, it doesn't count for the pressure.

V and T are fixed

This means the final pressure can be given by:

P2/P1 = n2/n1  

 with n2 = number moles of products

with n1 = number of moles of reactants

P2 = (6.0 mol*1.0 atm) / (3.0 mol )

P2 = Final pressure = 2.0 atm

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.