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2 years ago

12

Please help with 1 chemistry question thank you!

1 answer:

ale4655 [162]2 years ago

7 0

Here are the CORRECT names and molecular formulas

carbonate: $CO_3^{2-}$
bicarbonate: $HCO_3^{-}$

Choice 1 is incorrect

nitrite: $NO_2^{-}$
nitrate: $NO_3^{-}$

Choice 2 is incorrect

sulfite: $SO_3^{2-}$
sulfide: $S^{2-}$

Choice 3 is incorrect

By process of elimination, you can infer choice 4 is correct.

Actually, choice 4 is the only choice that displays the correct name and formula.

Have an awesome day! :)

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3 years ago

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2 years ago

Read 2 more answers

Calculate ΔH o rxn for the following: CH4(g) + Cl2(g) → CCl4(l) + HCl(g)[unbalanced] ΔH o f [CH4(g)] = −74.87 kJ/mol ΔH o f [CCl

anzhelika [568]

Answer: ΔH for the reaction is -277.4 kJ

Explanation:

The balanced chemical reaction is,

$CH_4(g)+Cl_2(g)\rightarrow CCl_4(l)+HCl(g)$

The expression for enthalpy change is,

$\Delta H=\sum [n\times \Delta H(products)]-\sum [n\times \Delta H(reactant)]$

$\Delta H=[(n_{CCl_4}\times \Delta H_{CCl_4})+(n_{HCl}\times B.E_{HCl}) ]-[(n_{CH_4}\times \Delta H_{CH_4})+n_{Cl_2}\times \Delta H_{Cl_2}]$

where,

n = number of moles

Now put all the given values in this expression, we get

$\Delta H=[(1\times -139)+(1\times -92.31) ]-[(1\times -74.87)+(1\times 121.0]$

$\Delta H=-277.4kJ$

Therefore, the enthalpy change for this reaction is, -277.4 kJ

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2 years ago

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3 years ago

If a sample of air in a school container was heated, would the percentage of oxygen in the air increase, decrease, or remain unc

Viktor [21]

Answer:

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Explanation:

Let's suppose we have a sample of air in a closed container. We heat the container and we want to predict what would happen to the pressure.

According to Gay-Lussac's law, the pressure of a gas is directly proportional to its absolute temperature.

Thus, if we increased the temperature of the air by heating it, its pressure would increase.

If a sample of air in a closed container was heated, the total pressure of the air would increase.

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2 years ago