Three volatile compounds X,Y, and Z each contain elements Q. The precent by weight of element Q in each compound was determined. Some of the data obtained are given below

Percent by weight Molecular
Compound of Element Q Weight

X 64.8% ?
Y 73.0% 104.
Z 59.3% 64.0
(a) the vapor density of compound X at 27 degress C and 750.mm Hg was determined to be 3.53 grams per litre. Calculate the molecular weight of compound X.

(b) Determine the mass of the element Q contained in 1.00 mole of each of the three compounds.

(c) Calculate the most probable value of the atomic weight of element Q

(d) Compound Z contains carbon, hydrogen, and element Q. When 1.00 gram of compound Z is oxidized and all of the carbon and hydrogen are converted to oxidized, 1.37 grams of CO2 and 0.281 gram of water are produced. determine the most prbable molecular formula of compound Z

(a) To calculate the molecular weight of compound X, we need to know its vapor density and the molar mass of the gas at the given conditions. The vapor density is given as 3.53 grams per liter, which means that one liter of the gas weighs 3.53 grams.

However, we are also given the percent by weight of element Q in compound X, which is 64.8%. This means that 64.8% of the total weight of compound X is accounted for by element Q.

To calculate the molecular weight of compound X, we need to find the weight of element Q in the compound. This can be done by multiplying the total weight of the compound (3.53 grams in this case) by the percent by weight of element Q (0.648). Therefore, the weight of element Q in compound X is:

Weight of element Q = 3.53 grams x 0.648 = 2.28344 grams

Now, we need to calculate the number of moles of element Q in compound X. To do this, we divide the weight of element Q by its molar mass.

Molar mass of element Q = (Weight of element Q) / (Percent by weight of element Q / 100)

Molar mass of element Q = 2.28344 grams / (64.8 / 100) = 3.52 grams

Therefore, the molecular weight of compound X is 3.52 grams per mole.

(b) To determine the mass of element Q contained in 1.00 mole of each compound, we need to use the given percent by weight of element Q for each compound.

For compound X, the percent by weight of element Q is 64.8%. Therefore, in 1.00 mole of compound X, the mass of element Q is:

Mass of element Q in 1.00 mole of compound X = (1.00 mole) x (64.8 / 100) = 0.648 moles

Similarly, for compound Y, the percent by weight of element Q is 73.0%. Therefore, in 1.00 mole of compound Y, the mass of element Q is:

Mass of element Q in 1.00 mole of compound Y = (1.00 mole) x (73.0 / 100) = 0.73 moles

For compound Z, the percent by weight of element Q is 59.3%. Therefore, in 1.00 mole of compound Z, the mass of element Q is:

Mass of element Q in 1.00 mole of compound Z = (1.00 mole) x (59.3 / 100) = 0.593 moles

(c) To calculate the most probable value of the atomic weight of element Q, we need to consider the masses of element Q in each of the compounds and calculate their average.

Average mass of element Q = (Mass of element Q in compound X + Mass of element Q in compound Y + Mass of element Q in compound Z) / 3

Average mass of element Q = (0.648 + 0.73 + 0.593) / 3 = 0.657 moles

Therefore, the most probable value of the atomic weight of element Q is 0.657 grams per mole.

(d) To determine the most probable molecular formula of compound Z, we need to consider the masses of carbon, hydrogen, and element Q in the oxidation reaction.

From the given data, 1.00 gram of compound Z produces 1.37 grams of CO2 and 0.281 grams of water when oxidized. This means that the total weight of carbon and hydrogen in the compound is:

Total weight of carbon and hydrogen = 1.37 grams (CO2) + 0.281 grams (H2O) = 1.651 grams

To calculate the percent by weight of carbon and hydrogen in compound Z, we divide the total weight of carbon and hydrogen by the total weight of compound Z:

Percent by weight of carbon and hydrogen = (Total weight of carbon and hydrogen / Total weight of compound Z) x 100

Percent by weight of carbon and hydrogen = (1.651 grams / 1.00 gram) x 100 = 165.1%

Since the total percent by weight of carbon and hydrogen exceeds 100%, there must be an error in the data or calculation. Please double-check the given information for compound Z to ensure accuracy in the calculations.