Answer:
Energy equals mass times the speed of light squared.
Explanation:
can i get brainliest? lol :) hope that helps
The electronic configuration of the elements which share the group, must have the last electron in same block..
Answer:
0.54 moles of N2
Explanation:
First remember to find the volume in moles, 1 mole equals 22.4 liters.
So now use the dimensional analysis to show your work.
12 liters of N2 * 1 mol /22.4 liters of N2
Now calculate this. 12 * 1/22.4 or 12/ 22.4
12/22.4 = 0.535714286.
12 has two significant digits.
With that, The answer rounds to 0.54.
So that the final answer is 0.54 moles.
Hope it helped!
First of all water (H2O) is made from 2 atoms of hydrogen and 1 atom of oxygen. A mole of water molecules would be 2 moles of hydrogen atoms plus 1 mole of oxygen atoms. So lets say x = 3m, m=1, and x=3, because 3 x 1 = 3 = x, and r = radius of drinking fountain's water dispense, and AOW = amount of water produced in a minute, and y = (x*(r*(AOW/r))... So Y = a, and a = answer... Meaning your answer is (y = (x*(r*(AOW/r)) )!
Answer:
0.22 g of CO2 were produced.
Explanation:
First, let's represent what is happening with an hypothetical chemical equation just to have a clearer vision of the presented process:
CaCO3 (aq) + 2 HAc (aq) → CaAc2 (aq) + H2O (l] + CO2 (g)
We have a tablet that has CaCO3 as the active ingredient that when combined with an acid, in this case represented as HAc, reacts producing a Calcium salt, water and carbon dioxide that will leave the solution as gas.
Having said that, we know that the initial mass of the reactants will have to maintain during the chemical reaction, or what is the same, the quantity of matter during the process will not change. So, if we have a tablet that weighs 0.853 g and we add an acid solution of 56.519 g, then we have that the initial mass of the reactants will be:
0.853 g from tablet + 56.519 g from acid solution = 57.372 g
This amount of matter should be the same after the reaction, but we know that the CO2 gas will leave the solution once it's formed, so considering that the resulting solution weighs 57.152 g we could calculate the mass of CO2 produced:
57.372 g of initial mass - 57.152 g of resulting solution = 0.22 g of CO2 that left the aqueous solution as gas.
