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3 years ago

Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)

Chemistry

1 answer:

Artemon [7]3 years ago

5 0

Answer:

Mg(s)+2HCl(aq)→MgCL2(aq)+H2(g), what mass of hydrogen will be obtained if 100 cm3 of 2.00 mol dm−3 HCl are added to 4.86 g of magnesium?

Explanation:

Moles of metal, = 4.86⋅g24.305⋅g⋅mol−1 = 0.200 mol.

Moles of HCl = 100⋅cm−3×2.00⋅mol⋅dm−3 = 0.200 mol

Clearly, the acid is in deficiency ; i.e. it is the limiting reagent, because the equation above specifies that that 2 equiv of HCl are required for each equiv of metal.

So if 0.200 mol acid react, then (by the stoichiometry), 1/2 this quantity, i.e. 0.100 mol of dihydrogen will evolve.

So, 0.100 mol dihydrogen are evolved; this has a mass of 0.100⋅mol×2.00⋅g⋅mol−1 = ??g.

If 1 mol dihydrogen gas occupies 24.5 dm3 at room temperature and pressure, what will be the VOLUME of gas evolved?

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Nimfa-mama [501]

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3 years ago

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°

miskamm [114]

<u>Answer:</u> The $\Delta H^o_{rxn}$ for the reaction is -1835 kJ.

<u>Explanation:</u>

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

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