Answer:
32.4 K
Explanation:
From the given parameters;
Initial pressure P1= 50.0 mmHg
Initial temperature T1= 540K
Final Temperature T2 = ?????
Final pressure P2=3 mmHg
Now using this relationship;
P1/T1 = P2/T2
We have; P1T2= P2T1
Hence;
T2= P2T1/P1
T2= 3 ×540/50.0
T2= 32.4 K
Warm areas since the molecules move faster when warm meaning more energy
The density of the sample is:
Density = mass / volume
Density = 9.85 / 0.675
Density = 14.6 g/cm³
If the sample has 95% gold, and 5% silver, its density should be:
0.95 x 19.3 + 0.05 x 10.5
Theoretical density = 18.9 g/cm³
The difference in theoretical and actual densities is very large, making it likely that the jeweler was not telling the truth.
1.icosahedralb2.helicalc3.complexa
Answer:
The theoretical yield of Cu(s) in moles is 60.15 moles
Explanation:
Step 1: Data given
Number of moles CuO = 70.8 moles
Number of moles NH3 = 40.1 moles
Molar mass CuO = 79.545 g/mol
Molar mass NH3 = 17.03 g/mol
Step 2: The balanced equation
3CuO(s) + 2NH3(g) → 3H2O(l) + 3Cu(s) + N2(g)
For 3 moles CuO we need 2 moles NH3 to produce 3 moles H2O, 3 moles Cu and 1 mol N2
NH3 is the limiting reactant. It will completely be consumed (40.1 moles). CuO is in excess. There will react 3/2 * 40.1 = 60.15 moles
There will remain 70.8 - 60.15 = 10.65 moles CuO
Step 3: Calculate moles Cu
For 3 moles CuO we need 2 moles NH3 to produce 3 moles H2O, 3 moles Cu and 1 mol N2
For 40.1 moles NH3 we'll have 60.15 moles Cu
The theoretical yield of Cu(s) in moles is 60.15 moles
