3. An industrial chemist introduces 2.0 atm H2 and 2.0 atm CO2 into a 1.00 L container at 25 ⁰C and then increases the temperature to 700 ⁰C. At that temperature, Kp = 0.534. How many grams of H2 are present when equilibrium is established? H2 (g) + CO2 (g) ⇌ H2O (g) + CO (g)

Explanation:

H₂ (g) + CO₂ (g) ⇌ H₂O (g) + CO (g)

2 atm pressure at 25° or 298 K . If temperature increases to 700°C or 973K

pressure = 2 x 973 / 298 = 6.53 atm

H₂ (g) + CO₂ (g) ⇌ H₂O (g) + CO (g)

6.53 - x    6.53 - x         x             x  

x² / ( 6.53 - x )²   = .534

x  / ( 6.53 - x )  = .73

x = 4.77 - .73 x

x = 2.76

pressure of hydrogen gas in equilibrium

= 6.53 - 2.76

= 3.77 atm

moles of hydrogen at this temperature and pressure

n = PV / RT

3.77 x 1 / .082 x 973

= .04725 mole

= .04725 x  2 gram

= .0945 gram

= 94.5 mili gram

answer

fusion: the energy source of stars. the energy released from the collapse of the gas into a protostar causes the center of the protostar to become extremely hot. when the core is hot enough, nuclear fusion commences. fusion is the process where two hydrogen atoms combine to form a helium atom, releasing energy.

hope it

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.