For a given reaction, adding a catalyst increases the rate of the reaction by

Chemistry

2 answers:

Ksju [112]3 years ago

8 0

Answer : Option 2) providing an alternate reaction pathway that has a lower activation energy

Explanation : When a catalyst is added to a chemical reaction it increases the rate of reaction by lowering the energy of activation. It provides an alternate pathway for a reaction to proceed with a lower Ea energy. Usually a catalyst never gets consumed in the reaction process. It will appear in the reaction mechanism steps but not in the overall reaction like reactants and products.

Andrej [43]3 years ago

6 0

The answer is (2) providing an alternate reaction pathway that has a lower activation energy. The lower activation energy will lead to the increase of rate of the reaction.

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For the following problem convert both the reactants to moles and balance chemical equationsThe reaction of 167 g Fe2O3 with 85.

saul85 [17]

Let's start by balancing the reaction:

$Fe_2O_3+CO\longrightarrow Fe+CO_2$

As we can see, C appears only on two comopunds, CO and CO₂, and since both have 1 C each, their coefficients have to be the same for C to be balanced. However, CO has 1 O and CO₂ has 2, so there is a difference of 1 O betwee them.

The other source of O is Fe₂O₃, that has 3 O. So, we must choose a coefficient for CO and CO₂ such that the difference between the numbers of O is a multiple of 3, that way we can fix this difference with the O from Fe₂O₃. So, we can put coefficients of 3 on both of them:

$Fe_2O_3+3CO\longrightarrow Fe+3CO_2$

That way, we maintained C balanced (3 on each side) and now we have 3 + 3 O on the left side and 6 O on the right side, so the same amount.

Now, we just have to calance Fe, but it is easy since we have it alone in Fe. Since we have 2 on the left side, it is enough to put a coefficient of 2 on Fe to get the balanced reaction:

$Fe_2O_3+3CO\longrightarrow2Fe+3CO_2$

Now, to convert from mass to number of moles, we need the molar masses of the reactants, which we can calculate from the atomic weights of the elemnts in each of them:

$M_{Fe_2O_3}=2\cdot M_{Fe}+3\cdot M_O=(2\cdot55.845+3\cdot15.9994)g/mol=159.6882g/mol$ $M_{CO}=1\cdot M_C+1\cdot M_O=(1\cdot12.0107+1\cdot15.9994)g/mol=28.0101g/mol$

Now, we can convert their masses to number of moles:

$\begin{gathered} M_{Fe_{2}O_{3}}=\frac{m_{Fe_2O_3}}{n_{Fe_{2}O_{3}}} \\ n_{Fe_2O_3}=\frac{m_{Fe_2O_3}}{M_{Fe_{2}O_{3}}}=\frac{167g}{159.6882g/mol}=1.045787\ldots mol \end{gathered}$ $\begin{gathered} M_{CO}=\frac{m_{CO}}{n_{CO}} \\ n_{CO}=\frac{m_{CO}}{M_{CO}}=\frac{85.8g}{28.0101g/mol}=3.063180\ldots mol \end{gathered}$

Now, to determine the limiting reactant, we need to divide both the number of mole by their coefficients on the balanced reaction, so we can see how many we need per reaction of each:

$\begin{gathered} Fe_2O_3\colon\frac{n_{Fe_2O_3}}{1}=\frac{1.045787\ldots mol}{1}=1.045787\ldots mol \\ CO\colon\frac{n_{CO}}{3}=\frac{3.063180\ldots mol}{3}=1.021060\ldots mol \end{gathered}$

Now, the limiting reactant is the one we have less number of moles per reaction. We can see that we have less CO than Fe₂O₃, so the limiting reactant is CO.

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Compare and contrast the use of U-238 and C-14 in absolute age dating

Talja [164]

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