how do you calculate this:
Calculate the mass of copper needed to displace 5.0g of silver from silver nitrate solution. (Relative Atomic Masses: Ag=108, Cu=63.5)
Eqn=Cu+2AgNO3->Cu(NO3)2+2Ag
How do you write a half equation?
Complete the half equation to show the oxidising action of bromine=
_I- ->I2___
Br2(aq)+2I-(aq)->2Br-(aq)+I2(aq)
I answered this question recently. Perhaps it was for another student. First, please clarify if this is 5.0 g Ag or 5.0 g AgNO3.
If it is 5.0 g Ag, convert 5.0 g Ag to mols, convert mols Ag to mols Cu using the coefficients in the balanced equation, then convert mols Cu to g Cu.
Remember mols = g/atomic mass for conversion of Ag to mols; then conversion of Cu to grams = mols Cu x atomic mass Cu.
The half equation is 2I^- ==> I2 + 2e
Post your work if you get stuck.
Mol=g/atomic mass of Ag wich is 5/108=0.046,usin the coefficients 1molCu produces 2molAg then 0.023mol produces 0.046mol,Cu mol multiplied by Cu atomic mass =1.472
Mol=g/atomic mass of Ag wich is 5/108=0.046,usin the coefficients 1molCu produces 2molAg then 0.023mol produces 0.046mol,Cu mol multiplied by Cu atomic mass =1.472
To calculate the mass of copper needed to displace 5.0g of silver from silver nitrate solution, you'll need to use stoichiometry and the relative atomic masses of copper (Cu) and silver (Ag). Here's the step-by-step breakdown:
1. Determine the molar mass of silver (Ag) and copper (Cu):
- The relative atomic mass of Ag = 108g/mol.
- The relative atomic mass of Cu = 63.5g/mol.
2. Write the balanced chemical equation for the reaction:
Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag
3. Use the stoichiometry of the reaction to convert from moles of silver (Ag) to moles of copper (Cu):
- According to the balanced equation, the ratio of moles of Ag to Cu is 2:1.
- Calculate the number of moles of Ag using its mass (5.0g) and molar mass (108g/mol):
Moles of Ag = Mass of Ag / Molar mass of Ag
4. Calculate the moles of Cu needed using the mole ratio from the balanced equation:
Moles of Cu = (Moles of Ag) / 2
5. Finally, calculate the mass of copper needed using its molar mass:
Mass of Cu = Moles of Cu * Molar mass of Cu
By following these steps, you can find the mass of copper needed to displace 5.0g of silver from the silver nitrate solution.
Regarding writing a half equation, let's take the example of the oxidizing action of bromine (Br2) on iodide ions (I-):
The given completed half equation is:
Br2(aq) + 2I-(aq) -> 2Br-(aq) + I2(aq)
The half equation represents either the oxidation or reduction reaction that takes place during a redox reaction. In this example, the half equation shows the oxidation of iodide ions (I-) to form iodine (I2).
Here's how you can write the half equation:
1. Identify the starting species and products involved in the redox reaction:
Starting species: I-
Products: I2
2. Write an unbalanced equation representing the transformation from the starting species to the product:
I- -> I2
3. Balance the equation by adding electrons (e-) to account for the change in oxidation states:
I- -> I2 + 2e-
4. Optionally, you can add spectator ions or states of matter (aq) to represent the reaction conditions.
By following these steps, you can write the half equation to show the oxidizing action of bromine on iodide ions, as shown above.