Two compounds that contain Cu and Cl have the following masses:
Cpd A: 32.10 g Cu and 17.90 g Cl
Cpd B: 23.64 g Cu and 26.37 g Cl
Are the compounds the same? If not, what is the lowest whole-number mass ratio of Cu that combines with a given mass of Cl?
Cu/Cl =
32.10/17.90 = 1.79
but
23.64/26.37 = .896
so no way the same compound
well .896/1 = 896/1000 = 448/500 = 224/250 = 112/125
Thank you so much!!
To determine if the compounds are the same, we can compare the mass ratio of Cu to Cl in each compound.
For Cpd A:
Mass of Cu = 32.10 g
Mass of Cl = 17.90 g
For Cpd B:
Mass of Cu = 23.64 g
Mass of Cl = 26.37 g
To find the lowest whole-number mass ratio of Cu to Cl, we need to divide the masses of each element by their respective atomic masses.
The atomic mass of Cu is approximately 63.55 g/mol, and the atomic mass of Cl is approximately 35.45 g/mol.
For Cpd A:
Number of moles of Cu = 32.10 g Cu / 63.55 g/mol ≈ 0.505 mol
Number of moles of Cl = 17.90 g Cl / 35.45 g/mol ≈ 0.505 mol
For Cpd B:
Number of moles of Cu = 23.64 g Cu / 63.55 g/mol ≈ 0.372 mol
Number of moles of Cl = 26.37 g Cl / 35.45 g/mol ≈ 0.743 mol
Comparing the moles of Cu to Cl, in Cpd A the ratio is approximately 0.505:0.505, which simplifies to 1:1.
In Cpd B, the ratio is approximately 0.372:0.743, which can be simplified to 1:2.
Since the mass ratio of Cu to Cl is different for the two compounds, they are not the same. The lowest whole-number mass ratio of Cu that combines with Cl is 1:1, as seen in Cpd A.
To determine whether the compounds are the same or not, we need to compare the mass ratios of Cu to Cl in both compounds.
For Compound A:
Mass of Cu: 32.10 g
Mass of Cl: 17.90 g
For Compound B:
Mass of Cu: 23.64 g
Mass of Cl: 26.37 g
To find the lowest whole-number mass ratio of Cu to Cl, we need to divide the masses of Cu and Cl in each compound by their respective molar masses.
The molar mass of Cu is 63.55 g/mol, and the molar mass of Cl is 35.45 g/mol.
For Compound A:
Cu mole ratio = (32.10 g Cu) / (63.55 g/mol Cu) = 0.505 mol Cu
Cl mole ratio = (17.90 g Cl) / (35.45 g/mol Cl) = 0.505 mol Cl
For Compound B:
Cu mole ratio = (23.64 g Cu) / (63.55 g/mol Cu) = 0.372 mol Cu
Cl mole ratio = (26.37 g Cl) / (35.45 g/mol Cl) = 0.743 mol Cl
Now, let's find the ratio of Cu to Cl in each compound by dividing the mole ratios:
For Compound A:
Cu:Cl ratio = (0.505 mol Cu) / (0.505 mol Cl) = 1:1
For Compound B:
Cu:Cl ratio = (0.372 mol Cu) / (0.743 mol Cl) = 1:2
The Cu:Cl ratio in Compound A is 1:1, while the Cu:Cl ratio in Compound B is 1:2. Therefore, the compounds are not the same.
To find the lowest whole-number mass ratio of Cu that combines with a given mass of Cl, we need to identify the common multiple between the Cu:Cl ratios of the two compounds.
The Cu:Cl ratio in Compound B is 1:2, which means that for every 1 mole of Cu, there are 2 moles of Cl.
To obtain a whole-number ratio, we can multiply this ratio by 2:
Cu:Cl ratio = 1:2 (multiplied by 2) = 2:4
Simplifying this ratio, we get:
Cu:Cl ratio = 1:2
Therefore, the lowest whole-number mass ratio of Cu that combines with a given mass of Cl is 1:2.