With the information given most likely in order to find the partial pressure of the gas produced you have to subtract the total air pressure in the collection flask by the atmospheric pressure since you assume that the flask started with atmospheric pressure when it was sealed and then the gas was added as the reaction took place increasing the pressure.
1.44atm-0.95 atm=0.49atm
Answer:
hydrogen atom when it drops from N 5 to N 2?
so, 275 kJ of energy is released when one mole of electrons "falls" from n = 5 to n = 2. E = hc/λ (this energy corresponds to the energy of one photon; the energy calculated in this problem is for one mole of photons so we will change this after we change the units from kJ to J)
Explanation:
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Answer:
2.24 Liters are in 4.4 grams of CO2 at STP
