A low-pressure weather system comes into the city of Denver. The atmospheric pressure is 693 mmHg.693 mmHg. If 78.0%78.0% of dry
air is nitrogen, what is the partial pressure of nitrogen in this low-pressure system?
1 answer:
Answer:
540.54 mmHg
Explanation:
We know that the partial pressure of a substance is defined as; Mole fraction * total pressure.
If the total amount of gases in the atmosphere is 100%, the mole fraction of nitrogen gas is now
78/100 = 0.78
Thus, partial pressure of nitrogen gas = 0.78 * 693 = 540.54 mmHg
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Answer:
10 Litre
Explanation:
Given that ::
v1 = 25L ; n1 = 1.5 mole ; v2 =? ; n2 = (1.5-0.9) = 0.6 mole
Using the relation :
(n2 * v1) / n1 = (n2 * v2) / n2
v2 = (n2 * v1) / n1
v2 = (0.6 mole * 25 Litre) / 1.5 mole
v2 = 15 / 1.5 litre
v2 = 10 Litre
OK in the case of hydrazine 14 grams of nitrogen combine with 2 gram of hydrogen and with ammonia 14 grams combine with 3 grams of hydrogen.
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Answer:
105.9888 g/mol
Explanation:
The molar mass of sodium carbonate is 105.9888 g/mol (grams per mole)
