Density = grams/milliliters
8.96 g/ml = grams Cu/50 ml
= 448 grams Cu
To make a 0.500 M solution of Cu(NO3)2, you'll need 0.500 moles in 1.00 L of solution. The molar mass of Cu(NO3)2 is 187.56 g/mol, so you would need 93.78 grams of Cu(NO3)2 to make 1.00 L of a 0.500 M solution.
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.
To find the number of molecules in 122 grams of Cu(NO3)2, we need to first calculate the molar mass of Cu(NO3)2. The molar mass of Cu(NO3)2 is approximately 187.55 g/mol. Next, we convert the given mass to moles using the molar mass. Finally, we use Avogadro's number (6.022 x 10^23) to find the number of molecules, which would be approximately 3.25 x 10^22 molecules.
Atomic mass of Cu is 63.55 a.m.u. , 63.55 g/mole(Cu is an element, not a molecule)
You need to know the density of copper, which is 8.96 g/cm3 at room temperature. Density = mass/volume. To solve for mass, the equation is manipulated so that mass = density x volume. 1mL = 1cm3, so 7.00mL Cu = 7.00cm3 Cu. Mass = 8.96g/cm3 x 7.00cm3 Cu =62.7g Cu
The atomic mass of Cu (Copper) is 63.546 amu (atomic mass unit).
To make a 0.500 M solution of Cu(NO3)2, you'll need 0.500 moles in 1.00 L of solution. The molar mass of Cu(NO3)2 is 187.56 g/mol, so you would need 93.78 grams of Cu(NO3)2 to make 1.00 L of a 0.500 M solution.
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.
To find the number of molecules in 122 grams of Cu(NO3)2, we need to first calculate the molar mass of Cu(NO3)2. The molar mass of Cu(NO3)2 is approximately 187.55 g/mol. Next, we convert the given mass to moles using the molar mass. Finally, we use Avogadro's number (6.022 x 10^23) to find the number of molecules, which would be approximately 3.25 x 10^22 molecules.
Atomic mass of Cu is 63.55 a.m.u. , 63.55 g/mole(Cu is an element, not a molecule)
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
You need to know the density of copper, which is 8.96 g/cm3 at room temperature. Density = mass/volume. To solve for mass, the equation is manipulated so that mass = density x volume. 1mL = 1cm3, so 7.00mL Cu = 7.00cm3 Cu. Mass = 8.96g/cm3 x 7.00cm3 Cu =62.7g Cu
The balanced equation for the reaction is: Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag Calculate the molar mass of Cu and Ag (Cu = 63.55 g/mol, Ag = 107.87 g/mol). Using the molar ratio of Cu to Ag (1:2), convert the mass of Cu to moles, then use the molar ratio to find the moles of Ag produced. Finally, convert moles of Ag to grams using the molar mass of Ag to find the grams of silver produced.
To find the mass of 1.20x10^28 atoms of copper (Cu), you need to first calculate the molar mass of copper (Cu), which is approximately 63.55 g/mol. Then, convert the number of atoms to moles by dividing by Avogadro's number (6.022 x 10^23 atoms/mol). Finally, convert moles to kilograms by multiplying by the molar mass and dividing by 1000 to get the mass in kilograms.
To find the mass in grams of 6.25 mol of copper(II) nitrate (Cu(NO3)2), you need to first calculate the molar mass of the compound using the periodic table. The molar mass of Cu(NO3)2 is 187.56 g/mol. Multiply the molar mass by the number of moles to find the mass: 6.25 mol * 187.56 g/mol = 1172.25 grams.
To determine the mass of copper (Cu) produced, you need to know the specific chemical reaction and the initial quantities of reactants involved. For example, in the reduction of copper(II) oxide (CuO) with hydrogen (Hâ‚‚), you would apply stoichiometry based on the balanced equation to find the mass of Cu produced. Once you have the moles of Cu calculated from the reactants, you can convert that to grams using the molar mass of copper (approximately 63.55 g/mol). Please provide more context or specific details about the reaction for a precise answer.
To find the mass of copper(II) nitrate, first calculate its molar mass: Cu(NO3)2 has a molar mass of approximately 187.56 g/mol. Then, multiply the molar mass by the number of moles to get the mass of 6.36 mol of copper(II) nitrate, which is approximately 1192.5 grams.