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Answer:
The partial pressure of nitrogen is 597.5 torr
Explanation:
Step 1: Data given
Mol fraction of N = 0.781
Mol fraction of O = 0.209
Mol fraction Ar = 0.010
Atmospheric pressure = 765.0 torr
The partial pressure is given by Pi = Xi * Pt
⇒ χ
i = the mole fraction of gas i in the mixture
⇒ P
total = the total pressure of the mixture
Step 2: Calculate the partial pressure of nitrogen
P(N) = mol fraction of N * atmospheric pressure
P(N) = 0.781 * 765.0 torr = 597.5 torr
The partial pressure of nitrogen is 597.5 torr
Answer: Plate movement is thought to be driven by a combination of the motion of the seafloor away from spreading ridges due to variations in topography and density changes in the crust.
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Answer:
Correct option is B. It shows the ratio of elements in the compound.
Explanation:
Empirical formula is the simplest form of the chemical formula. It shows the simplest ratio of atoms in compounds. It is determined by %age of each element.
Answer: Option (b) and (d) are correct.
Explanation:
An equilibrium reaction is defined as the reaction in which rate of forward reaction equals rate of backward reaction.
A photosynthesis reaction is the reaction in which plants in the presence of sunlight, water, and carbon dioxide make their own food.
- The amount of carbon dioxide consumed will be equal to the rate of formation of oxygen into the atmosphere.
Hence, the statement rate of formation of
is equal to the rate of formation of
is true.
- Concentration of oxygen may remain constant but it will not decrease. Hence, the statement concentration of
will begin decreasing, is false.
- As both oxygen and carbon dioxide are present in an equilibrium reaction, So, their concentration will not change.
Hence, the statement concentrations of
and
will not change, is true.
- Concentration of carbon dioxide and oxygen will also depend on the limiting reagent. So, it is not necessary that the concentrations of
and
will be equal.
Some amount of carbon dioxide might escape out into the air.
Hence, the statement concentrations of
and
will be equal, is false.