When 1.375 g of copper (II) oxide is reduced on heating in a current of hydrogen, the weight of copper remaining after the react
1 answer:
Answer:
20.11% of oxygen
Explanation:
The reaction is:
2CuO ⇒ 2Cu + O2
If you have an initial amoung of a sample, thi may be have impurities, so you have to start from products to know what you had at the begining.
to make a relation between reagents and products you need to change the mass to mol, then you can relate them with the molar ratio.
Now you have the initial amount of oxygen, to convert to percent you must divide the mass of oxygen between the mass of the sample and multiply by 100
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Answer:
0.012mol
Explanation:
1.
Given parameters:
Pressure in the balloon = 1.25atm
Volume of the balloon = 2.5L
Unknown:
Number of moles = ?
Solution:
We are going to used the combined gas law to solve this problem.
PV = nRT
P is the pressure
V is the volume
n is the number of moles
R is the gas constant = 0.082atmdm³mol⁻¹K⁻¹
Insert the parameters and solve;
1.25 x 2.5 = n x 0.082 x 285
n = 0.13mol
The number of moles is 0.13mol
2.
Given parameters:
Pressure = 16torr;
to atm is ;
760torr = 1atm
16torr = = 0.02atm
Volume = 12L
Temperature = 253K
Using the ideal gas law;
PV = nRT
0.02x12 = n x 0.082 x 253
n = 0.012mol