Chemistry, 01.04.2020 19:21 val452

For the reaction H2(g) + I2(g) 2HI(g), Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75  10-3 M at 445ºC, which one of these statements is true? A) The system is at equilibrium, thus no concentration changes will occur. B) The concentrations of HI and I2 will increase as the system approaches equilibrium. C) The concentration of HI will increase as the system approaches equilibrium. D) The concentrations of H2 and HI will fall as the system moves toward equilibrium. E) The concentrations of H2 and I2 will increase as the system approaches equilibrium

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Answer from: diego481

The reaction approaching towards equilibrium results in the increase in HI concentration. Thus, option C is correct.

The balanced chemical equation has been given as:

$\rm H_2\;+\;I_2\;\rightarrow\;2\;HI$

The equilibrium has been the condition when the concentration of reactants and products in the reaction has been equal. The given condition has equal concentration of all the compounds in the mixture.

The reactant concentration has been the sum of concentration of hydrogen and iodine.Thus, the concentration of reactants has been higher than the concentration of product HI.

Thus, on moving towards the equilibrium condition, the concentration of HI increases. Thus, option C is correct.

For more information about equilibrium, refer to the link:

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Answer from: reaperdraws

C) The concentration of HI will increase as the system approaches equilibrium.

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_c

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

$H_2(g)+I_2(g)\rightarrow 2HI(g)$

The expression for Q_c is written as:

$Q_c=\frac{[HI]^2}{[H_2]^1[I_2]^1}$

$Q_c=\frac{(1.75\times 10^{-3})^2}{(1.75\times 10^{-3})^1\times (1.75\times 10^{-3})^1}$

Q_c=1.00

K_c=50.2

Thus as $K_{eq}Q$ , the reaction will shift towards the right i.e. towards the product side.

Answer from: Quest

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –

6.022

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,

will have a gram-molecular weight of 352g.

Answer from: Quest

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