Answer:
See below.
Explanation:
The mass of octane in the sample of gasoline is 0.02851 * 482.6 = 13.759 g of octane.
The balanced equation is:
2C8H18(l) + 25O2(g) ----> 16CO2(g) + 18H2O(g)
From the equation, using atomic masses:
228.29 g of octane forms 704 g of CO2 and 324.3 g of H2O
So the mass of CO2 formed from the combustion of 13.759 g of octane = (704 * 13.759) / 228.29
= 42.43 g of CO2.
Amount of water = 324.3 * 13.759) / 228.29
= 19.55 g of H2O.
Neon is an element because it is a pure atom
Answer:
1.18 moles of gas
Explanation:
3.00 moles of gas are pumped into a 1.00L rigid container with a pressure of 1.98 atm. The gas is released from the container until the pressure is 0.78 atm, how many moles of gas remain in the container?
for the sealed rigid container, the pressure is directly proportional to the amount of gas
3.00moles/1.98 atm = ? moles/0.78 atm
? = 3.00 X 0.78/1.98 =1.18 moles of gas
It is A; <span>[He] 2s</span>²<span> 2p</span>² is another way to put it
