Answer:
Volume of dry gas at STP = 0.432 liters or 432 ml
Explanation:
Given:
Pressure (P) = 740 mmHg - 24 mmHg = 716 mmHg
Temperature (t) = 25 degrees C + 273 K = 298 K
500 ml = 0.5 l
Find:
Volume of dry gas at STP
Computation:
[P1][V1] / T1 = [P2][V2] / T2
[716][0.5] / 298 K = [760][ x Liters] / 273 K
x = 0.432 Liters
Volume of dry gas at STP = 0.432 liters or 432 ml
The answer to this question will be C
Answer:
See explanation
Explanation:
The periodic table shows the atomic number and mass number of each element.
We know that the atomic number shows;
- The number of protons in the nucleus of the atom
- The number of electrons in the neutral atom of the element.
So we obtain the number of protons and electrons by looking at the atomic number shown in the periodic table.
We also know that;
Mass number = Number of protons + number of neutrons
Since number of protons = atomic number of the atom
Number of neutrons = Mass number - atomic number
Hence we obtain the number of protons by subtracting the atomic number from the mass number given in the periodic table.
the number of moles of oxygen required are 0.08 mol. The volume of oxygen that is required to react can be calculated by the formula shown below. Substitute the values in equation (II). Hence, the volume of oxygen required to react with 3.6 L hydrogen is 1.8L . I hope this helps if not I’m sorry
