Answer:
22.656 grams of oxygen gas are there in a 2.3L tank at 7.5 atm and 24° C
Explanation:
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law:
P * V = n * R * T
where R is the molar constant of the gases and n the number of moles.
In this case you know:
- R= 0.082
- T= 24 °C= 297 °K (being 0°C=273°K)
Replacing:
Solving:
n=0.708 moles
Knowing that oxygen gas is a diatomic gas of molecular form O₂ and its mass is 32 g / mole, you can apply the following rule of three: if 1 mole contains 32 grams, 0.708 moles, how much mass will it have?
mass= 22.656 grams
<u><em>22.656 grams of oxygen gas are there in a 2.3L tank at 7.5 atm and 24° C</em></u>
Answer:
Two moles of hydrogen gas combine with one mole of oxygen gas to produce two moles of water.
Explanation:
This is the required amount of each element to synthesize water. The equation has been balanced using coefficients.
The correct answer is Seafloor Spreading
Give me brainliest if it is correct!
A solution with hydroxide ion concentration of 4.15 x10^-6 m is basic and has a hydrogen ion concentration of 2.41 x10^-9 M
we well know thaat (H^+) (OH^-) = 1 x10^-14
by making H^+ concentration the subject of the formula
H^+ = 1 x10^-14/OH^-
H^+= 1 x10^-14/4.15 x10^-6 = 2.41 x10^-9 M
the solution is basic since OH^- ion is for basic solution