2.2 moles of O2 will be produced by the decomposition of 4.4 moles of water.
Answer:
10 atm.
Explanation:
Using the combined gas law equation as follows;
P1V1/T1 = P2V2/T2
Where;
P1 = initial pressure (atm)
P2 = final pressure (atm)
V1 = initial volume (L)
V2 = final volume (L)
T1 = initial temperature (K)
T2 = final temperature (K)
According to the information provided in this question,
P1 = 5 atm
P2 = ?
V1 = 4L
V2 = 2L
T1 = 25°C = 25 + 273 = 298K
T2 = 25°C = 298K
Using P1V1/T1 = P2V2/T2
5 × 4/298 = P2 × 2/298
20/298 = 2P2/298
Cross multiply
298 × 20 = 298 × 2P2
5960 = 596P2
P2 = 5960 ÷ 596
P2 = 10 atm.
False. It is a fluid as it is in its liquid state possessing qualities of a liquid just that it is viscious
Explanation:
here's the answer to your question
Finding percent composition is fairly easy. You only need to divide the mass of an element by the total mass of the compound. We can do this one element at a time.
First, let's find the total mass by using the masses of the elements given on the periodic table.
7 x 12.011 (mass of Carbon) = 84.077
5 x 1.008 (mass of Hydrogen) = 5.04
3 x 14.007 (mass of Nitrogen) = 42.021
6 x 15.999 (mass of Oxygen) = 95.994
Add all of those pieces together.
84.077 + 5.04 + 42.021 + 95.994 = 227.132 g/mol is your total. Since we also just found the mass of each individual element, the next step will be very easy.
Carbon: 84.077 / 227.132 = 0.37016 ≈ 37.01 %
Hydrogen: 5.04 / 227.132 = 0.022189 ≈ 2.22 %
Nitrogen: 42.021 / 227.132 = 0.185 ≈ 18.5 %
Oxygen: 95.994 / 227.132 = 0.42263 ≈ 42.26 %
You can check your work by making sure they add up to 100%. The ones I just found add up to 99.99, which is close enough. A small difference (no more than 0.03 in my experience) is just a matter of where you rounded your numbers.
