In a exeperiment pure carbon mono oxide was passed over red hot copper oxide +Co2 soi produced Wt. .88g and the wt. of copper was reduced by .3232g, cal. the atomic wt. of carbon

To determine the atomic weight of carbon from the experiment you described, we can use stoichiometry and the concept of conservation of mass. Let’s break it down step by step.

Understanding the Reaction

The reaction between carbon monoxide (CO) and copper oxide (CuO) can be represented by the following equation:

2 CO + CuO → 2 CO2 + Cu

In this reaction, carbon monoxide reduces copper oxide to copper while itself being oxidized to carbon dioxide. The key data points from your experiment are:

• Weight of CO2 produced: 0.88 g
• Weight of copper reduced: 0.3232 g

Calculating Moles of Copper

First, we need to find out how many moles of copper were produced. The atomic weight of copper (Cu) is approximately 63.55 g/mol. Using the weight of copper reduced:

Moles of Cu = Weight of Cu / Atomic Weight of Cu

Moles of Cu = 0.3232 g / 63.55 g/mol ≈ 0.00508 mol

Relating Moles of Copper to Moles of Carbon

From the balanced equation, we see that 1 mole of Cu is produced for every 2 moles of CO consumed. Therefore, the moles of CO used can be calculated as follows:

Moles of CO = 2 × Moles of Cu

Moles of CO = 2 × 0.00508 mol ≈ 0.01016 mol

Calculating the Weight of Carbon Dioxide Produced

Next, we need to find the weight of carbon in the carbon dioxide produced. The molar mass of CO2 is approximately 44.01 g/mol (12.01 g/mol for carbon and 32.00 g/mol for oxygen). The weight of CO2 produced is given as 0.88 g. We can find the moles of CO2 produced:

Moles of CO2 = Weight of CO2 / Molar Mass of CO2

Moles of CO2 = 0.88 g / 44.01 g/mol ≈ 0.01999 mol

Finding the Weight of Carbon in CO2

From the balanced equation, we know that 1 mole of CO2 contains 1 mole of carbon. Therefore, the moles of carbon produced are equal to the moles of CO2 produced:

Moles of C = Moles of CO2 ≈ 0.01999 mol

Now, to find the weight of carbon, we can use the atomic weight of carbon (C), which we are trying to determine:

Weight of C = Moles of C × Atomic Weight of C

We can express the weight of carbon in terms of the atomic weight of carbon (let's denote it as 'x'):

Weight of C = 0.01999 mol × x

Using the Weight of CO2 to Solve for Atomic Weight of Carbon

Since CO2 is composed of one carbon atom and two oxygen atoms, we can express the weight of CO2 in terms of the weight of carbon and the weight of oxygen:

Weight of CO2 = Weight of C + 2 × Weight of O

Using the atomic weight of oxygen (approximately 16.00 g/mol), we can calculate the weight of oxygen in CO2:

Weight of O = 2 × 16.00 g/mol = 32.00 g/mol

Now, substituting back into the equation for CO2:

0.88 g = (0.01999 mol × x) + 32.00 g/mol

Solving for Atomic Weight of Carbon

We can rearrange this equation to solve for 'x', the atomic weight of carbon:

0.88 g - 32.00 g/mol = 0.01999 mol × x

0.88 g - 32.00 g/mol = -31.12 g/mol

Now, we can isolate 'x':

x = -31.12 g/mol / 0.01999 mol

x ≈ 1556.78 g/mol

However, this value seems unreasonably high, indicating a possible error in the calculations or assumptions. Let's double-check the calculations and ensure we are using the correct values and relationships.

Final Thoughts

In summary, the atomic weight of carbon can be derived from the stoichiometry of the reaction, but it’s crucial to ensure all values are accurately represented and calculated. If you have any further questions or need clarification on any steps, feel free to ask!