A combustion reaction of an will generally produce CO2 and H20 -- carbon dioxide and water and/or an oxide
looking at the combustion material C2H2, you know that the end products will be CO2 and H20, so the question is how much of each will you get
well, look at the total amount of carbon atoms, 2 C2, which means a total of 4 carbon atoms in this reaction, since only CO2 has carbon atoms, that means there must be 4 CO2 as an end product and 4 CO2 will use up 4 of 5 O2 molecule leaving only 1 O2 molecule for the H2 reaction.
now O2 has a total of 2 oxygen molecules whereas H20 has only a single oxygen molecule, hence the end product must have 2 H20
check that the H atoms balance out on both sides
Answer:3.5 days is awfully precise and waxing gibbous is awfully vague.Let’s just make sure we understand our terminology. Waxing means getting fatter and gibbous means fat. A waxing gibbous moon lasts for approximately 7 days from the first quarter phase right up to the full moon phase.By 3.5 days I’m assuming you mean half a week and simplifying the lunar phases to 28 days exactly.So we have:Day 0 New moon.Day 7 First quarter.Day 14 Full moon.Day 21 Third quarter.Day 28 New Moon.Between day 0 - 7 we have the waxing crescent phase.Between day 7–14 we have the waxing gibbous phase.Between day 14–21 we have the waning gibbous phase.Between day 21–28 we have the waning crescent phase.So 3.5 days from day 7 would take us to day 10.5 which would still leave us in the waxing gibbous phase. 3.5 days after day 10.5 would take us to the full moon or over into the waning gibbous phase since the full moon lasts only an instant.
Explanation:
Answer:
Mass = 179.9 g
Explanation:
Given data:
Volume of solution = 450 mL
Molarity of solution = 2.00 M
Mass in gram required = ?
Solution:
Volume of solution = 450 mL× 1 L / 1000 mL = 0.45 L
Molarity = number of moles of solute/ Volume of solution in L
2.00 M = number of moles of solute / 0.45 L
Number of moles of solute = 2.00 M × 0.45 L
M = mol/L
number of moles of solute = 0.9 mol
Mass of CaBr₂ in gram:
Mass = number of moles × molar mass
Mass = 0.9 mol ×199.89 g/mol
Mass = 179.9 g
