Given:
Mass of X = 0.858 g
Mass of CO produced = 2.63 g
Mass of HO produced = 1.28 g

To determine:
The lowest molecular mass X can have

Solution:

1. Find the moles of CO and HO produced using their respective molar masses:

Molar mass of CO = 12.01 + 15.99 = 28 g/mol
Moles of CO = 2.63 g / 28 g/mol = 0.094 mol

Molar mass of HO = 1.01 + 15.99 = 18.01 g/mol
Moles of HO = 1.28 g / 18.01 g/mol = 0.071 mol

2. Determine the limiting reactant:

The balanced chemical equation for the combustion of X is:

CₓHᵧ + (x + y/4)O₂ → xCO₂ + (y/2)H₂O

From the equation, we can see that 1 mole of X produces x moles of CO₂ and y/2 moles of H₂O. Therefore, the theoretical yield of CO and HO can be calculated as:

Theoretical yield of CO = x × moles of X
Theoretical yield of HO = (y/2) × moles of X

Using the masses of CO and HO produced, we can calculate the actual yield of each product:

Actual yield of CO = 2.63 g
Actual yield of HO = 1.28 g

Using the molar masses of CO and HO, we can calculate the number of moles produced:

Moles of CO produced = 0.094 mol
Moles of HO produced = 0.071 mol

To determine the limiting reactant, we need to compare the moles of CO and HO produced to their theoretical yields:

Theoretical yield of CO = x × moles of X
= x/2 × moles of X (since 1 mole of X produces x/2 moles of CO)
Theoretical yield of HO = (y/2) × moles of X

Comparing the moles of CO and HO produced to their theoretical yields:

Moles of CO produced = 0.094 mol
Theoretical yield of CO = x/2 × moles of X

Moles of HO produced = 0.071 mol
Theoretical yield of HO = (y/2) × moles of X

We need to find which value of x and y will give the lowest molecular mass of X.

3. Determine the molecular formula of X:

To determine the molecular formula of X, we need to find the values of x and y that satisfy the following conditions:

1. The moles of CO produced must be equal to the theoretical yield of CO:
0.094 mol = x/2 × moles of X

2. The moles of HO produced must be equal to the theoretical yield of HO:
0.071 mol = (y/2) × moles of X

To find the lowest molecular mass of X, we need to try different values of x and y. We can start with the smallest whole number values and increase until we find a combination that satisfies both conditions.

Let's try x = 2 and y = 2:

0.094 mol = 2/2 ×

Given:
- Mass of compound X = 0.858 g
- Mass of CO produced = 2.63 g
- Mass of HO produced = 1.28 g

We need to find the lowest molecular mass X can have.

Approach:
1. Write the balanced chemical equation for the combustion of compound X.
2. Calculate the number of moles of CO and HO produced.
3. Calculate the number of moles of C and H in compound X.
4. Use the molecular formula of X to calculate its molecular mass.
5. Find the lowest molecular mass X can have.

Solution:
1. Balanced chemical equation for the combustion of compound X:

CₓHᵧOᵨ + (x + y/4 - r/2)O₂ → xCO₂ + (y/2)H₂O

From the balanced equation, we can see that for every x moles of compound X, we get x moles of CO₂ and y/2 moles of H₂O.

2. Calculation of the number of moles of CO and HO produced:

Number of moles of CO produced = Mass of CO produced / Molar mass of CO

Molar mass of CO = 12.01 + 15.99 = 28 g/mol

Number of moles of CO produced = 2.63 g / 28 g/mol = 0.094 moles

Number of moles of HO produced = Mass of HO produced / Molar mass of HO

Molar mass of HO = 1.01 + 15.99 = 18.01 g/mol

Number of moles of HO produced = 1.28 g / 18.01 g/mol = 0.071 moles

3. Calculation of the number of moles of C and H in compound X:

From the balanced equation, we can see that for every x moles of compound X, we get x moles of CO₂.

Number of moles of CO2 produced = Number of moles of CO produced = 0.094 moles

Since one mole of CO₂ contains one mole of C, we can say that the number of moles of C in compound X is also 0.094 moles.

From the balanced equation, we can see that for every x moles of compound X, we get y/2 moles of H₂O.

Number of moles of H₂O produced = Number of moles of HO produced / 0.5

Number of moles of H₂O produced = 0.071 moles / 0.5 = 0.142 moles

Since one mole of H₂O contains two moles of H, we can say that the number of moles of H in compound X is 0.284 moles.

4. Use the molecular formula of X to calculate its molecular mass:

Let the molecular formula of compound X be CₐHᵦOᵩ

The molar mass of X can be calculated as follows:

Molar mass of X = (a x 12.01) + (b x 1.01) + (o x 15.99)

5. Find the lowest molecular mass X can have:

We know that X contains 0.094 moles of C and 0.284 moles of H.

From the