52.0 divided by 65 g/mol gives you 0.8mol
I would say carpool why because you don't know what the hybrid car runs on
<span />
Hello!
To start off, we must look at atomic masses. Atoms all have different weights, so we must first find hydrogen and oxygen's atomic masses.
Oxygen: 16.00 amu
Hydrogen: 1.01 amu
Now, moving on to the weight of water itself. Water has the formula of H20, with two hydrogen atoms and one oxygen. Therefore, <u>add up the amus to get the weight of one molecule of water.</u>
1.01 + 1.01 + 16.00 = 18.02 amu
Now, to see the ratio of each component. Since hydrogen weighs a total of 2.02 amu (1.01 + 1.01) in the entire atom, we can state that hydrogen makes up about 0.112 of the weight of water. Now apply that ratio to 16 g, and solve.
0.112x = 16
142.857143 = x
So therefore, about 143 grams of water are made when 16g of hydrogen reacts with excess oxygen.
Hope this helps!
<span>The correct answer is ideal gas law.
when the ideal gas law formula is:
PV = nRT ,
when P is the pressure.
V is the volume.
and R is the ideal gas constant.
T is the temperature.
and n is the number of moles.
So, this is the law which relates pressure, temperature, volume and number of moles . and this law state that 1 mole of an ideal gas will occupy a volume V = 22.4 L</span>
Answer:
mass
Explanation:
The amount of kinetic energy an object has, depends on its mass and its speed.
