Question

In: Chemistry

Using the below data: Mass (g) of copper gluconate: 1.0 g Mass (g) of wrapper: 0.6...

Using the below data:

Mass (g) of copper gluconate: 1.0 g

Mass (g) of wrapper: 0.6 g

Mass (g) of wrapper + Cu: 0.9 g

Mass (g) of Cu: 0.3 g

Mass (g) of gluconate: 0.7 g

1. Determine the chemical formula of copper gluconate?

2. Calculate the percent composition of copper and the percent composition of gluconate in the compound copper gluconate?

3. Create a Experimental Chemical Formula:

Solutions

Expert Solution

Mass of gluconate = 0.7g

And mass of Cu = 0.3g

Answer1.

Chemical formula of compound is determine from first convert into mole

Mole = given mass / molecular weight

Mole of Cu = 0.3g/63.546g/mole = 0.004720989519mole

Mole of gluconate is = 0.7g/195.127g/mole = 0.003588mole.

But we know that reaction is

Cu2+ + 2gluconate = Cu2+(gluconate)2

Hence above gluconate is limiting reagent and mole of Cu 2+ is use in half of the mole of gluconate = 0.003587407/2 = 0.001794mole

Or mass of copper use is = mole of Cu use in reaction * molecular weight of Cu

Mass of copper is = 0.001794mole *63.536g/mole = 0.11398g use

Hence chemical formula is Cu2+(gluconate)2

Answer 2

Mass of total compound is = 0.11398g of Cu + 0.7g mass of gluconate = 0.81398g

Mass percent of Cu = 0.11398g*100/0.81398g= 14.00275%

Mass percent of gluconate is = 0.7g*100/0.81398g = 85.99719%

Answer 3

Experimental chemical formula is same

Cu2+(gluconate)2


Related Solutions

Lab Results: 1 gram of Copper Gluconate; Mass of Cu 0.2g; Mass of gluconate 0.4 g...
Lab Results: 1 gram of Copper Gluconate; Mass of Cu 0.2g; Mass of gluconate 0.4 g 1. Using your own lab results, show your calculations for your moles of copper produced. You must show all work to receive credit. 2. Using your own lab results, show your calculations for your moles of gluconate. You must show all work to receive credit. 3. Using your own lab results, determine the chemical formula of copper gluconate. You must show all work (not...
Determine the number of moles of copper in the copper gluconate using your results. experiment 1:...
Determine the number of moles of copper in the copper gluconate using your results. experiment 1: determining the chemical formula for copper gluconate Data Sheet Table 2: Mass Compound Mass (g)                        Copper Gluconate       1.9g Aluminum Cup + Copper 2.0g -Aluminum Cup 0.6g Copper 0.6g Table 3: Givens Name Given Copper Gluconate Formula Cu(C6H11Ox)n Molecular Weight of C 12.01 g/mol Molecular Weight of H 1.008 g/mol Molecular Weight of O 16.00 g/mol Molecular Weight of Cu 63.55 g/mol Table 4:...
In an experiment, 698 g of water is in a copper calorimeter cup of mass 204...
In an experiment, 698 g of water is in a copper calorimeter cup of mass 204 g. The cup and the water are at an initial temperature of 11.3 oC. An unknown material with a mass of 411 g at a temperature of 421.8 oC is placed in the water. The system reaches thermal equilibrium at 31.1 oC. What is the specific heat of the unknown material?
In an experiment, 426 g of water is in a copper calorimeter cup of mass 205...
In an experiment, 426 g of water is in a copper calorimeter cup of mass 205 g. The cup and the water are at an initial temperature of 10.9 oC. An unknown material with a mass of 361 g at a temperature of 296.1 oC is placed in the water. The system reaches thermal equilibrium at 36.1 oC. What is the specific heat of the unknown material? units = J/kg-C
An alloy contains 97% by mass aluminium and 3% by mass copper. 8. Using 100 kg...
An alloy contains 97% by mass aluminium and 3% by mass copper. 8. Using 100 kg of material as the starting point, what proportion of the atoms are copper?
1. What mass of water is needed to dissolve 43.5 g of copper (II) chloride to...
1. What mass of water is needed to dissolve 43.5 g of copper (II) chloride to prepare a 0.521 molal solution? 2. Calculate the boiling point of a solution made from 224 g of magnesium chloride dissolved in 625 g of water. kb= 0.512 degrees celsius/m
Find ΔH° for the complete combustion of gaseous methoxyethane , C3H8O(g) , using the data below....
Find ΔH° for the complete combustion of gaseous methoxyethane , C3H8O(g) , using the data below. C(s) + O2(g) → CO2(g) ΔH°= -393.52 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔH°= -285.83 kJ/mol 3C(s) + 4H2(g) + ½O2(g) → C3H8O(g) ΔH°= -216.4 kJ/mol ΔH° for the complete combustion of gaseous methoxyethane
Calculate specific rotation, %ee, and %R and %S using the data below Mass of product: 0.171...
Calculate specific rotation, %ee, and %R and %S using the data below Mass of product: 0.171 g Volume of solution: 5.00 mL Path length: 1.000 dm Observed rotation: 0.95 Thanks !!
Table 1: Mass Data Mass (g) Trial 1 Trial 2 Trial 3 Water 48.0 g 48.5...
Table 1: Mass Data Mass (g) Trial 1 Trial 2 Trial 3 Water 48.0 g 48.5 g 48.3 g Metal Strip 36.9 g 37.0 g 37.2 g Table 2: Specific Heat Data Time (minutes) Temperature (°C) Trial 1 Trial 2 Trial 3 Initial 35.1 C 35.6 C 35.6 C 5 minutes 35.3 C 36.4 C 35.8 C 6 minutes 35.0 C 36.0 C 35.4 C 7 minutes 34.6 C 35.7 C 35.4 C 8 minutes 34.6 C 35.5 C 35.3...
Methanol is manufactured by the partial combustion of methane under pressure, using a copper catalyst: CH4(g)...
Methanol is manufactured by the partial combustion of methane under pressure, using a copper catalyst: CH4(g) + ½ O2(g) → CH3OH(l) Enthalpies of combustion are (in kJ mol-1): CH4(g), -881 CH3OH(l), -726 Calculate the standard enthalpy change for the manufacture of 1 mole methanol by the reaction CH4(g) + ½ O2(g) → CH3OH(l) Follow the procedures based on Hess’s Law: First write down the reactions corresponding to the enthalpies of combustion you have been given, reverse one of the equations...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT