Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 25.0 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 ∘C) is mixed with 22.2 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 ∘C). The reaction produces 26.2 L of hydrogen gas measured at STPWhat is the percent yield of the reaction?

The % yield of this reaction is 61.9 %

Explanation:

Step 1: Data given

Volume of methane = 25.0 L

Pressure of methane = 732 torr = 732 /760 atm = 0.9631579 atm

Temperature = 25.0 °C = 298 K

Volume of water vapor = 22.2 L

Pressure of water vapor = 704 torr = 704/760 atm = 0.92631579 atm

Temperature = 125 °C 398 K

The reaction produces 26.2 L hydrogen gas

Step 2: The balanced equation

CH4(g)+H2O(g)→CO(g)+3H2(g)

Step 3: Calculate moles methane

p*V = n*R*T

n  =(p*V)/(R*T)

⇒with n = the moles of methane = TO BE DETERMINED

⇒with p= the pressure of methane = 732 torr = 0.9631579 atm

⇒with V = the volume of methane = 25.0 L

⇒with R = the gas constant =0.08206 L*atm/mol*K

⇒with T = the temperature = 298 K

n = (0.9631579 * 25.0) / (0.08206*298)

n = 0.984668 moles

Step 4: Calculate moles H2O

p*V = n*R*T

n  =(p*V)/(R*T)

⇒with n = the moles of H2O= TO BE DETERMINED

⇒with p= the pressure of methane = 704 torr = 0.92631579  atm

⇒with V = the volume of methane = 22.2 L

⇒with R = the gas constant =0.08206 L*atm/mol*K

⇒with T = the temperature = 398 K

n = (0.92631579  * 22.2 )/(0.08206 * 398) = 0.62965 mol H2O

Step 5: Calculate moles H2

CH4(g) + H2O(g) ⇄ CO(g) + 3H2(g)

For 1 mol CH4 we need 1 mol H2O to produce 1 mol CO and 3 moles H2

H2O is the limiting reactant. It will completely be consumed. (0.62965 moles). Methane is in excess. There will react 0.62965 moles. There will remain  0.984668 - 0.62965 = 0.355018 moles methane

For 0.62965 moles H2O we'll have 3*0.62965 = 1.88895 moles H2

Step 6: Calculate volume H2

p*V = n*R*T

V= (n*R*T)/p

⇒with V = the volume of H2 = TO BE DETERMINED

⇒with n = the moles of H2 produced = 1.88895 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 273K

⇒with p = the pressure of H2 = 1.0 atm

V = (1.88895 * 0.08206 * 273) / 1.0

V = 42.32 L

Step 7: Calculate the percent yield

% yield = (actual yield / theoretical yield) * 100 %

% yield = (26.2 / 42.32) * 100 %

% yield = 61.9 %

The % yield of this reaction is 61.9 %

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.

one negative thing it that it can kill water animals. another negative thing is it can cause the destruction of ecosystem. one way water pollution can be reduced is to conserve energy.