To solve this we assume
that the gas is an ideal gas. Then, we can use the ideal gas equation which is
expressed as PV = nRT. At a constant temperature and number of moles of the gas
the product of PV is equal to some constant. At another set of condition of
temperature, the constant is still the same. Calculations are as follows:
P1V1 =P2V2
P2 = P1 x V1 / V2
P2 = 2.0 x 1.5 / 3
<span>P2 = 1 atm</span>
Thermodynamics, Nuclear Physics, Quantum Physics, Astronomy and Astrophysics
34g C * ( 1 mol / 12.0107 ) * ( 1 mol H2 / 1 mol C ) * ( <span>2.01588 g / 1 mol H2 ) = 5.70657164028741 g H2 = 5.7 g H2
Convert grams of C to moles of C using the given amount of grams and the molar mass ( 12.0107 g/mol ).
Gather the mole ratio from the coefficients in the balanced equation and multiply by the ratio.
Convert moles of H2 to grams of H2 </span> using the given amount of grams and the molar mass ( 2.01588 g/mol )<span>.
Revise your answer to have the correct number of significant figures. </span>
Answer:
<u>Nucleus</u> - The central part of the atom containing protons and neutrons.
<u>Electron</u> - A positively charged particle located in the nucleus of an atom.
<u>Proton</u> - A positively charged particle located in the nucleus of an atom.
<u>Electron Cloud</u> - The area of the at surrounding the nucleus where electrons can be found.
<u>Neutron</u> - a negatively charged particle that orbits the nucleus of an atom.