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

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explanation:

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.