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Heat reaclionIhermechemicul cquivalence 10) Consider the following reaction: 2 Mg (s) 0.(g1 - 2 MsO (s) AH? ; 1204KJ Is this reactionCxowkztmicor endolhermic? Expla...

Question

Heat reaclionIhermechemicul cquivalence 10) Consider the following reaction: 2 Mg (s) 0.(g1 - 2 MsO (s) AH? ; 1204KJ Is this reactionCxowkztmicor endolhermic? ExplainWst the enthalpy chinge pcT muJc ofM;O formed?enthalpy change for the formation ot4 *of Mgo?Whatenthalpy change for the decomposition of 3of MgO?D) What makch hcut produced? of Mg reacts with excess Oz (E) howE) When _micb heal produced? mol of Mg reacts with 2 mol 0z (g} hov F) WhenSpecitc Her

Heat reaclion Ihermechemicul cquivalence 10) Consider the following reaction: 2 Mg (s) 0.(g1 - 2 MsO (s) AH? ; 1204KJ Is this reactionCxowkztmicor endolhermic? Explain Wst the enthalpy chinge pcT muJc ofM;O formed? enthalpy change for the formation ot4 * of Mgo? What enthalpy change for the decomposition of 3 of MgO? D) What makch hcut produced? of Mg reacts with excess Oz (E) how E) When _ micb heal produced? mol of Mg reacts with 2 mol 0z (g} hov F) When Specitc Her



Answers

Consider the following reaction:
$$2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s) \quad \Delta H=-1204 \mathrm{kJ}$$
(a) Is this reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 3.55 $\mathrm{g}$ of $\mathrm{Mg}(s)$ reacts at constant pressure. (c) How many grams of MgO are produced during an enthalpy change of $-234 \mathrm{kJ}$ ? (d) How many kilojoules of heat are absorbed when 40.3 $\mathrm{g}$ of MgO(s) is decomposed into $\mathrm{Mg}(s)$ and $\mathrm{O}_{2}(g)$ at con stant pressure?

In this reaction, we are asked to do some calculations for the reaction I have listed on the top of the page. It's a reaction between elemental magnesium and oxygen. The first question is, is this an exo or endo thermic reaction? Since the heat term is negative. This is an exo thermic reaction. Again, we know that because it is a negative delta H. Our 2nd question says, calculate the amount of heat. So I'm just gonna make elk the heat four, 3.55 g a magnesium reacting at constant pressure. This is a pretty easy problem to set up. It's just like uh I guess you just called a basic straight geometry problem and I've got it right. Hang on up there it is, add a written down. But I've got so many papers So it's 3.55 g of magnesium. We're going to convert grams of magnesium, two moles of magnesium using the molar mass. The more massive magnesium is 24.31 g. And then we're gonna multiply this by our heat term, Which is negative 1204 killer jewels per And notice I'm used to moles Of Magnesium because I've got a coefficient of two. That's a four. If you can't tell there were three significant figures in my given. So the answer is negative 87 0.9 killer jewels. That is beat. We will switch colors for C for C. Were asked to do another calculation how many grams of M. G. O. Magnesium oxide are produced during an an therapy change of negative 2. 34 killer jewels. Also a simple straight geometric Problem -34 Killer Jewels. Yeah, Just by four there. Yeah. Mhm I think I've got the wrong. No, that was right. And I've got negative 12 oh four kg jewels per. Again, I'm going to have to moles of magnesium oxide because There's a coefficient of two and the molar mass of magnesium oxide, It's 40.30 grams per mall. Once again, 3, 3 significant figures and I got 15.7 grams of magnesium oxide. And that is part seat last but not least. We've got a part D. I will switch colors again. And indeed we are asked how many kilograms of heat Given 43 g of magnesium oxide. So we're gonna start with our 40 point three g. Again, the molar masses, 40.30 grams per mole. I'm going to leave the ngos off Now. I've got my 1204 -12 or four killer jewels per two malls M. G. O. That should be it. And I got 602 killer jewels. And I'm going to circle this exo thermic. There are the four answers. I can't get my problems stopped here.

If you look, you can see that Delta H. Is negative. Therefore this reaction is excellent thermal. If we start with 2.4 g of magnesium, we can figure out the energy will simply change grams of magnesium, two moles of magnesium and then use our balanced equation to relate moles of magnesium to kill a jewels. So one mall of Magnesium is 24.31 g. And according to our equation, two moles of magnesium releases as many killer jewels. So this will give us negative 59 killer jewels and it's negative. So it's released. If we release 96 killer jewels, let's figure out how much MG. Oh we make. So I'm going to change killer jewels, two moles of NGO. We can use our balanced equation to relate those and then I'll change moles of M. G. O. two g of NGO. Okay, so according to our equation, very two moles of NGO, We released 1204 killer jewels. Then one mall is 43 1 g. So this would be 6.43 g of M. G. O. We're in this last one we're reversing the reaction. So our delta H. We have to change its sign. It's now 1200 killer jewels For two moles of NGO on behalf of that for one mole. So 7.50 g of R. m. g. o. We'll change grams to moles and then malls to kill the jewels. So now it's 2, 2 positive, 12 4 And still 1 to 43, 1 Mhm. So it would absorb 112 killer jewels. Yeah

So let's think of a simple reaction where we have some reactant are gonna be broken down into two products. Product one and product too. Now, what we know about this reaction is it has a positive and full P value. Delta H is positive. This positive entropy value tells us that this reaction is endo thermic and we know that it's Endo thermic. In order for this reaction to occur, he must be absorbed. It must be introduced to the system in order for this to occur. So if we have a positive Delta H and we know it is Endo thermic, we know this reaction absorbs heat. So say we have the reverse reaction. We have the same two products being combined together to form the original reactant. Now, if we think about it, the reverse reaction is gonna have the opposite sign and magnitude of the previous simple P. So this Delta H here is going to be negative, right? Because we know going this way, he must be absorbed, but going the opposite way. We know that it's going to give off heat, and if it's giving off, he it's exile. Thermic and its ample p will be negative. Now the value will also be the opposite. No, I'm sorry. The sign will be the opposite, but the value will be the same. For example, if you have the Delta h of one problem say is 100 killer jewels and then you dio the reverse reaction. The Delta H will be negative. 100 killer jewels. You see, we keep the same value. It's the same amount of heat given or absorb. What changes is the sign. And this is true if you start with a reaction that gives off, he has a negative entropy. If you do the birth, it's going to absorb heat this time. So we know when we reverse reaction. Were always flipping the sign. So let's consider the temple p when we have 5.35 moles of CO two reacting with magnesium oxide. So in this case, we're doing the reverse reaction that we see up here because we're combining the two products here to get the original reactive. So we know that we have to change the sign of the M pulpy. And if we think about it, the info p here, which would be negative 117 0.3 Killah jewels is written for one wall. And if we want to multiply by the 5.35 Moles of CO two that we have because we know that since everything's bounced, if we have 5.35 moles of CO two will have the same number of moles of the magnesium oxide and as well as the magnesium carbonate. Here we dio a simple multiplication to cancel moles and we get negative 627 0.56 killing jewels. And so this is the end puppy of the reverse reaction when we are given a set number of moles. Now, if we're given some mass value instead, we have to do the exact same thing. We have to dio one quick conversion first because we have the reaction right now and that's given for one mole. But here were given a mass value. So we did have to convert this massive co 22 moles. And we know that all we have to do is divide by the molar mass. So we have 44.1 grams per mole of co two. This is grams that cancels and we're left with 0.807 moles of C 02 And now we're gonna do the same thing as we did before. We have our temple p of the reverse reaction, which is equal to 117.3. And this is killer jewels, Permal. And then we have a Moeller value to cancel out with. So we have to point e 07 moles. These cancel out and our final entropy is negative. 94.62 killing jewels.

That's the balanced equation can very written as twice off on G solid autos is in gas bomb, which is yourself. And she well, the standard and to beef permission. ISS standard. And they'll be Yeah, formations fall. The edge is not off. Send your doors will be minus 601.6 collegial my market.


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