your question is incomplete or incorrectly worded You want to know how much copper is in 100 grams of an unknown sample. The unknown could be made of anything, it may not even contain copper. You should include more information in your question
To determine the number of grams of Cu(NO3)2 produced, you need to consider the molar ratio between Cu(NO3)2 and Cu. Firstly, convert the 4.2 grams of Cu to moles using the molar mass of Cu. Then, use the balanced chemical equation to find the moles of Cu(NO3)2 produced. Finally, convert the moles of Cu(NO3)2 to grams using its molar mass.
Multiply 564 grams of copper by 1 mole over the atomic mass of copper (represented in grams). 564 g Cu * 1 mol Cu / (atomic mass) g Cu The atomic mass is located on the periodic table and represented in atomic units. The same value is used here, but with the unit as grams.
B. 24.6 grams. To find this, you must first calculate the molar mass of Cu and CuS. This will give an idea of the mole ratio between Cu and CuS. Then, you can use stoichiometry to determine that 24.6 grams of Cu₂S will yield 10.0 grams of Cu.
1 mol of an element is equal to it's atomic weight, but with grams instead of amu (or daltons) as the unit. For example, with copper (Cu), 63.5 amu is its rough atomic weight, which means it weighs roughly 63.5g per mol. Then we just need to divide through. 63.5 x 0.345 = 21.9g
The balanced chemical equation for the reaction between copper (Cu) and nitric acid (HNO3) is Cu + 4HNO3 -> Cu(NO3)2 + 2NO2 + 2H2O. From the equation, it can be seen that 1 mol of Cu reacts with 4 mol of HNO3. Therefore, to react with 2.0 mol of HNO3, 0.5 mol of Cu is needed. The molar mass of Cu is approximately 63.5 g/mol, so 0.5 mol of Cu would be equivalent to 31.75 grams.
To determine the number of grams of Cu(NO3)2 produced, you need to consider the molar ratio between Cu(NO3)2 and Cu. Firstly, convert the 4.2 grams of Cu to moles using the molar mass of Cu. Then, use the balanced chemical equation to find the moles of Cu(NO3)2 produced. Finally, convert the moles of Cu(NO3)2 to grams using its molar mass.
The atomic mass of Copper is 63.5 grams One mole of any element has a mass equal to the atomic mass. 0.75 grams of Cu = x moles of Cu 63.5 grams of Cu = 1 mole of Cu Set up a proportion and solve for x Divide 0.75 / 63.5 = x /1 0.75 ÷ 63.5 = x
For this you need the atomic mass of Cu. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel.2068 grams Cu / (63.5 grams) = 32.6 moles Cu
Multiply cu m by 1,000,000 to convert to cu cm. 1 cu m = 1 m * 1 m * 1m = 100 cm * 100 cm * 100 cm = 1000000 cu cm
Multiply 564 grams of copper by 1 mole over the atomic mass of copper (represented in grams). 564 g Cu * 1 mol Cu / (atomic mass) g Cu The atomic mass is located on the periodic table and represented in atomic units. The same value is used here, but with the unit as grams.
B. 24.6 grams. To find this, you must first calculate the molar mass of Cu and CuS. This will give an idea of the mole ratio between Cu and CuS. Then, you can use stoichiometry to determine that 24.6 grams of Cu₂S will yield 10.0 grams of Cu.
There are 748 gallons in 100 cu ft.
4,5 moles of copper are equivalent to 285,957 g.
1 mol of an element is equal to it's atomic weight, but with grams instead of amu (or daltons) as the unit. For example, with copper (Cu), 63.5 amu is its rough atomic weight, which means it weighs roughly 63.5g per mol. Then we just need to divide through. 63.5 x 0.345 = 21.9g
bob Marley
The balanced chemical equation for the reaction between copper (Cu) and nitric acid (HNO3) is Cu + 4HNO3 -> Cu(NO3)2 + 2NO2 + 2H2O. From the equation, it can be seen that 1 mol of Cu reacts with 4 mol of HNO3. Therefore, to react with 2.0 mol of HNO3, 0.5 mol of Cu is needed. The molar mass of Cu is approximately 63.5 g/mol, so 0.5 mol of Cu would be equivalent to 31.75 grams.
25' x 4' = 100 sq ft. 100 sq ft x 1' = 100 cu ft. 100 cu ft x 2 = 200 cu ft.