The following reaction was carried out in a 2.50 L reaction vessel at 1100 K:C(s)+H2O(g)⇌CO(g)+H2(g)If during the course of the reaction, the vessel is found to contain 6.75 mol of C, 13.5 mol of H2O, 3.10 mol of CO, and 9.00 mol of H2, what is the reaction quotient Q?Enter the reaction quotient numerically

The reaction quatient Q is 0.306

Explanation:

Step 1: data given

Volume = 2.50 L

Temperature = 1100 K

Number of moles C = 6.75 moles

Number of moles H2O = 13.5 moles

Number of moles CO = 3.10 moles

Number of moles H2 = 9.00 moles

Step 2: The balanced equation

C(s)+H2O(g)⇌CO(g)+H2(g)

Step 3: Calculate the concentration

Concentration = moles / volume

[C] = 6.75 moles / 2.5 L

[C] = 2.7 M

[H20] = 13.5 moles / 2.5 L

[H2O] = 5.4 M

[CO] = 3.10 moles / 2.5 L

[CO] = 1.24 M

[H2] = 9.00 moles / 2.5 L

[H2]= 3.6 M

Step 4: Calculate Q

Q = [CO][H2] / [C][H2O]

Q = (1.24 * 3.6)/(2.7*5.4)

Q = 0.306

The reaction quatient Q is 0.306

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.