Once the system reaches equilibrium at 675°C additionally H2 is added in the temperature is held constant which statement best describes how this affects the value of K

The given question is incomplete. The complete question is :

Once the system reaches equilibrium at 675°C additionally H2 is added in the temperature is held constant which statement best describes how this affects the value of K

1. The value of K increases because the formation of products is favoured.

2. The value of K decreases because the formation of reactants .

3. The value of K remains unchanged because the temperature remained constant.

4. The value of K cannot be determined as until the equilibrium concentrations are determined.

Answer : The value of K remains unchanged because the temperature remained constant.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as K.

K has a definite value for every chemical reaction at a particular temperature.

K is independent of initial concentrations of the reactants.

K changes with the temperature change.

K depends on the nature of the reaction.

Thus as temperature is held constant,  the value of K also remains constant.

i think its 5049.

i hope this !

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2