The given question is incomplete, the complete question is:
A reaction between liquid reactants takes place at 10.0 °c in a sealed, evacuated vessel with a measured volume of 35.0 L. Measurements show that the reaction produced 28. g of dinitrogen difluoride gas. Calculate the pressure of dinitrogen difluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits. pressure:atm
Answer:
The correct answer is 0.28 atm.
Explanation:
The temperature mentioned in the given reaction is 10 degree C, which after conversion becomes 283 Kelvin (273+10 = 283K).
The volume mentioned in the reaction is 35 Liters.
The reaction produced 28 grams of dinitrogen difluoride gas (N2F2). The n or the no of moles of the gas can be determined with the help of the formula:
moles of N2F2 = mass/molar mass
= 28/66 (molar mass of N2F2 is 66 g/mol)
= 0.424
The pressure of the gas can be determined by using the equation of the ideal gas law, that is, PV = nRT
P * 35 = 0.424 * 0.0821 * 283
P = 0.28 atm
Answer:
CO2
Explanation:
(I Just took the test)
At STP 1 mol=22.4 Liters, so we now know that it is asking for which of the gasses has a molar mass of 44, and CO2 is th only one with that molar mass
Answer:
Does lithium oxide react with hydrochloric acid?
Explanation:
Lithium Hydroxide reacts with acids to produce a Lithium salt: Hydrochloric Acid + Lithium Hydroxide → Lithium Chloride + Water. HCl + LiOH → LiCl + H2O. ... H2SO4 + 2LiOH → Li2SO4 + 2H2O
is this what you wanted to know?
Answer:
Conduction, Convection, and Radiation .......
Answer:
because not enough of the parent isotope remains to measure accurately. because not enough of the daughter product has formed to be detectable.
Explanation:
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