The following information is given for ether, C2H5OC2H5, at 1atm:

boiling point = 34.6oC Hvap(34.6oC) = 26.5 kJ/mol
melting point = -116oC Hfus(-116oC) = 7.27 kJ/mol
specific heat liquid = 2.32 J/goC

At a pressure of 1 atm, what is H in kJ for the process of condensing a 33.7 g sample of gaseous ether at its normal boiling point of 34.6 oC

I am not sure how to start this

q = mass ether x delta Hvap = ?

I would convert 33.7g ether to mole and use that for mass which will match the unit for delta Hvap in kJ/mol. q will have units of kJ.

To solve this problem, we need to calculate the enthalpy change (H) for the process of condensing the gaseous ether sample at its normal boiling point of 34.6°C.

1. Determine the number of moles of the gaseous ether sample:
Number of moles = Mass / Molar mass

The molar mass of ether (C2H5OC2H5) can be calculated by summing the atomic masses of its constituent elements:
C: 2 atoms x atomic mass of carbon
H: 6 atoms x atomic mass of hydrogen
O: 1 atom x atomic mass of oxygen

Atomic mass of carbon = 12.01 g/mol
Atomic mass of hydrogen = 1.008 g/mol
Atomic mass of oxygen = 16.00 g/mol

Molar mass of ether = (2 x 12.01) + (6 x 1.008) + (1 x 16.00)

Plug in the values and calculate the molar mass.

2. Using the boiling point information, calculate the amount of heat required to vaporize the gaseous ether sample at its boiling point:
Q = n x Hvap

n = number of moles of the sample (from step 1)
Hvap = molar heat of vaporization at the boiling point (26.5 kJ/mol)

Plug in the values and calculate the heat (Q) in joules.

3. Convert the heat value obtained in step 2 from joules to kilojoules:
1 kJ = 1000 J

Divide the heat value by 1000 to obtain the heat (H) in kJ.

Make sure to carry out the calculations step by step and retain all the decimal places for more accurate results.

To find the enthalpy change (ΔH) for the process of condensing a 33.7 g sample of gaseous ether at its normal boiling point of 34.6 oC, you need to consider the following steps:

Step 1: Calculate the energy required to heat the gaseous ether from its boiling point to its final temperature.

Given:
- Boiling point (T1) = 34.6 oC
- Mass of the sample (m) = 33.7 g
- Specific heat capacity of the liquid (c) = 2.32 J/goC

The heat energy required to heat the sample can be calculated using the formula:

Q1 = mcΔT

where ΔT = final temperature - initial temperature.

ΔT = Tfinal - T1
ΔT = T1 - T1 (since it is at its boiling point)
ΔT = 0

Therefore, Q1 = mcΔT = 0 J

Step 2: Calculate the energy required for the phase change from the gaseous state to the liquid state.

Given:
- Heat of vaporization at boiling point (Hvap) = 26.5 kJ/mol

We need to convert the mass of the sample to moles by using the molar mass of ether.

Molar mass of ether (C2H5OC2H5) = (2 * 12.01 g/mol) + (6 * 1.01 g/mol) + (2 * 16.00 g/mol)
= 74.12 g/mol

Number of moles (n) = mass/molar mass
n = 33.7 g / 74.12 g/mol

Now, we can calculate the energy required for the phase change:

Q2 = nHvap

Step 3: Calculate the total enthalpy change (ΔH) by summing up the energy from Step 1 and Step 2.

ΔH = Q1 + Q2

Finally, we can substitute the values and perform the calculations to find the enthalpy change in kJ.

Note: Make sure to convert units if necessary to maintain consistency throughout the calculations.