Answer:
Percent yield = 94.5%
Theoretical yield = 26.89 g
Explanation:
Given data:
Mass of copper = 12.5 g
Mass of copper chloride produced = 25.4 g
Theoretical yield = ?
Percent yield = ?
Solution:
Cu + Cl₂ → CuCl₂
Number of moles of Copper:
Number of moles = mass/ molar mass
Number of moles = 12.5 g/ 63.55 g/mol
Number of moles = 0.2 mol
Now we will compare the moles of copper with copper chloride.
Cu : CuCl₂
1 : 1
0.2 : 0.2
Theoretical yield:
Mass of copper chloride:
Mass = Number of moles × molar mass
Mass = 0.2 mol × 134.45 g/mol
Mass = 26.89 g
Percent yield:
Percent yield = Actual yield / theoretical yield × 100
Percent yield = 25.4 g/26.89 g × 100
Percent yield = 94.5%
1,3,2
The coefficient multiplied by the subscript will give you how many atoms of the element there are.
So, if we plug in 1,3,2
There will be 2 Nitrogen and 6 Hydrogen in the reactants side of the equation. To balance this on the other side, we must put a 2 in order to get 2 Nitrogen and 6 Hydrogen again.
Answer:
16.82 L.
Explanation:
- We can use the general law of ideal gas: PV = nRT.
where, P is the pressure of the gas in atm (P = 1.0 atm, STP conditions).
V is the volume of the gas in L (V = ??? L).
n is the no. of moles of the gas in mol (n = mass/molar mass = (12.0 g)/(15.99 g/mol) = 0.7505 mol).
R is the general gas constant (R = 0.0821 L.atm/mol.K),
T is the temperature of the gas in K (T = 0.0°C + 273 = 273.0 K, STP conditions).
<em>∴ V = nRT/P</em> = (0.7505 mol)(0.0821 L.atm/mol.K)(273.0 K)/(1.0 atm) = <em>16.82 L.</em>
Answer: it they are both in the same place
Explanation:I don’t know and don’t care loser
