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1 year ago

Match the action to the effect on the equilibrium position for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). (3 points)

Chemistry

1 answer:

AleksandrR [38]1 year ago

5 0

Answer:

1. Adding hydrogen gas, b. shift to the right
2. Adding a catalyst, c. No effect
3. Decreasing the pressure, a. shift to the left

Explanation:

Hydrogen gas can be rewritten as H2. Whenever you add something to an equilibrium expression, it will shift to whichever side does not have this. So, since the reactant side has 3 moles of H2, adding more H2 to the reaction will shift to the products side, since there is no H2 there.

Adding a catalyst has no effect on equilibrium reactions.

When decreasing the pressure, equilibrium will shift to the side with the greater number of moles of gas. In this case, there are 4 moles of gas on the left, and 2 on the right, so it would shift to the left.

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mass of gasoline= density * volume
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3 years ago

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Marianna [84]

Answer:

Explanation:

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The solubility product of PbI2 is 7.9x10^-9. What is the molar solubility of PbI2 in distilled water?

Agata [3.3K]

<u>Answer:</u> The molar solubility of $PbI_2$ is $1.25\times 10^{-3}mol/L$

<u>Explanation:</u>

Solubility is defined as the maximum amount of solute that can be dissolved in a solvent at equilibrium.

Solubility product is defined as the product of concentration of ions present in a solution each raised to the power its stoichiometric ratio.

The balanced equilibrium reaction for the ionization of calcium fluoride follows:

$PbI_2\rightleftharpoons Pb^{2+}+2I^-$

s 2s

The expression for solubility constant for this reaction will be:

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We are given:

$K_{sp}=7.9\times 10^{-9}$

Putting values in above equation, we get:

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2 years ago

In the reaction C + O2 → CO2, 18 g of carbon react with oxygen to produce 72 g of carbon dioxide. What mass of oxygen would be n

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Stoichiomety:

1 moles of C + 1 mol of O2 = 1 mol of CO2

multiply each # of moles times the atomic molar mass of the compund to find the relation is weights

Atomic or molar weights:

C: 12 g/mol
O2: 2 * 16 g/mol = 32 g/mol
CO2 = 12 g/mol + 2* 16 g/mol = 44 g/mol

Stoichiometry:

12 g of C react with 32 g of O2 to produce 44 g of CO2

Then 18 g of C will react with: 18 * 32/ 12 g of Oxygen = 48 g of Oxygen

And the result will be 12 g of C + 48 g of O2 = 60 g of CO2.

You cannot obtain 72 g of CO2 from 18 g of C.

May be they just pretended that you use the law of consrvation of mass and say that you need 72 g - 18g = 54 g. But it violates the proportion of C and O2 in the CO2 and is not possible.

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