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Problem- Upon decomposition, one sample of magnesium fluoride produced 1.66kg of magnesium and 2.58kg of fluorine. A second sample produced 1.32kg of magnesium.
How much fluorine in grams did the second sample produce?
I am in hurry anyone is there provide me the answer in quick phase
you heat a 454 gram aluminum pot to cook some mac amp cheese. if the temperaure changes from 22.0oc to 275oc and the
The hydration of norbornene and the bromination of trans-cinnamic acid are both examples of additions across a double bond. How many new stereocenters were generated in the hydration
Calcium reacts with oxygen to make calcium oxide, CaO. What is the theoretical yield (g) of CaO(s) that could be prepared from 7.91 g of Ca(s) and 2.04 g of O2(g)
Refer to the following abbreviated standard reduciton potential table. Which one is the of the following reactions would be considered NON=SPONTANEOUS
The daily energy requirement for an active adult human is around 2500 calories per day. A nutritional calorie is equal to 4.2 kJ of energy. If each ATP contains -30 kJ/mol under standard conditions, how many molecules of ATP does the body require ..
Identify the statements that accurately explain how hydrogen ion concentration relates to energy production in oxidative phosphorylation.
What is the internal energy change for the system if 969 joules of heat flows into the system from the surroundings and 253 joules of work is done by the system on the surroundings
Explain what is the hydronium-ion concentration in a solution formed by combining 150mL of 0.10 M NaOH with 50mL of 0.30 M HCl
A person is exposed for three days to identical amounts of two different nuclides that emit positrons of roughly equal energy. The half-life of nuclide A is 18.5 days and the half-life of nuclide B is 255 days.
ttwo containers are connected by a stopcock. gas a is at pressure 202 kpa while gas b is at pressure 140 kpawhat will
which of the following is always spontaneous A. C2H6O + 3O2 = 2CO2 + 3H2O; delta H is smaller than 0 B. the sublimation of dry ice ( CO2) C. the freezing of water (H2O) D. the formation of water from its gaseous elements D. None of the above.
The most common error students make during a titration is that they add extra NaOH past the endpoint causing the solution to change a dark pink color.
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