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Consider the following reaction:2 Na + 2HCl → 2 NaCl + H2How many mols of hydrogen gas (H2) can be produced ifyou begin with 1.070 grams of HCl:...

Question

Consider the following reaction:2 Na + 2HCl → 2 NaCl + H2How many mols of hydrogen gas (H2) can be produced ifyou begin with 1.070 grams of HCl:

Consider the following reaction: 2 Na + 2HCl → 2 NaCl + H2 How many mols of hydrogen gas (H2) can be produced if you begin with 1.070 grams of HCl:



Answers

Given the reaction of hydrogen and chlorine gases, calculate the moles of hydrogen that react to produce $5.00 \mathrm{~mol}$ of $\mathrm{HCl}$. $$\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g)$$

This question is a strike geometry and ideal gas law question where you need to review your concepts, you learned of stoke eom a tree and apply them with the ideal gas law. It's like geometry requires a balanced chemical reaction. The reaction is sodium with hydrochloric acid producing sodium chloride and hydrogen gas. When balanced, two moles of each produced two moles sodium chloride and one mole hydrogen gas. So if we have 3.50 g of sodium, we can convert that into moles of sodium by dividing by the molar mass of sodium and then convert the moles of sodium into moles of hydrogen gas. This is the story geometry part of this question. Once we know the moles of hydrogen gas, we can then use the ideal gas law with the temperature and pressure of the hydrogen gas to calculate its volume rearrangement of the ideal gas law gives us V. Is equal to NRT overpay. So we'll take in the moles of hydrogen. We just calculated multiply it by our, multiply it by the kelvin temperature Celsius plus 2 73 divided by the pressure in ATM, and we get 1.83 liters of hydrogen being produced.

In this problem. We have 3.5 grams of sodium metal reacting with HCL to form on A C. L and hydrogen gas and were asked if I ng to the volume that hydrogen gas will take up at a temperature of 18 degrees Celsius and pressure of 180.995 atmospheres. So first, uh, we need to find the moles of hydrogen gas so we can use the ideal gas equation, which is PV equals NRT. But in order to find the moles of hydrogen, we first have to find the mold of sodium that were given. So we'll take that 3.5 grams of sodium and its molecular weight, which you can find on the periodic table, is 23 grams Permal. So we'll have one mold over 23 grams. It'll cancel. These grams will be left with mole as our unit, and we have 0.152 moles of sodium and then Teoh convert that two moles of hydrogen. We're gonna look at this, uh, balance equation that we've got up here so to multi sodium per one mole of hydrogen, so one mole hydrogen over two moles sodium. So we can cancel or moles of sodium. And we're left with 0.76 moles of hydrogen. So now we can use our ideal gas equation. But first, we need to make sure everything is in the correct units. So we have moles over here for end. That's good. Are pressure is an atmospheres. But then we need to convert our temperature into Calvin. So to convert from Celsius to Calvin, we add to 73. So that gives us a temperature of to 91 Calvin. So now we can do our ideal gas equation. So our pressure is 0.995 atmospheres. Volume is what we're solving for and we just saw before is zero point through 76 moles are is the ideal gas constant is 0.8 to 1 leader a T M. Over mole. Okay. And our temperature is 2 91 Okay, like we just saw before. So if we do the math on this side, we will find out that we have 1.816 over here, and then our moles canceled. Our Kelvin's canceled. So we have a leader a t m. Over here. We've got that 0.995 a t. M. Times our volume, you can cancel the atmospheres. And if we divide 1.816 by 0.95 like I changed a whole lot will get one point 82 leaders as our volume.

This is a limiting reactant problem which, you know, because you were given masses or amounts of both reactions and asked if on the product we don't know which reaction is going to run out first. But to compare, we can't compare mass. We can only compare mold because this reaction is has a mole to mole ratios, is how articles react. So we're gonna start by converting two moles. We're gonna divide each of these masses by the molar mass of each substance for hydrogen gas. This is 2.2 grams for every one mole of hydrogen gas that's gonna be equal to 1.76 moles of each to We're gonna receipt Pete the same process for chlorine gas, which has a much greater molar mass. In this case, that's 70.91 grams for every one mole of seal too dividing eight. But 70 gives 0.1 to 6 more of feel to it. We're gonna actually answer the first question. Second question first, like comparing these ratios, notice that these react again in a 1 to 1 ratio. So that means that if I have all of this 1.76 moles react. It's going to need 1.76 moles of feel, too. But clearly we do not have enough TL to to make this happen. Alternatively, you can think that so clearly, feel, too, is the limiting reactant thought of it another way. You could say that the 0.1 to 6 more chlorine needs 0.1 to 6 moles of H two, but we have way more than that available. Thus, we see that H two is the excess reactant. Chlorine is limiting reactive, no matter which way I look at it that the answer, the first question or the second question feel, too, is the limiting reactant? Because it is the limiting reaction. It determines how much product hydrogen chloride is informed. How much product is for based on these multiple ratios, there's twice as many moles of hydrogen chloride as is chlorine gas. So if I multiply this value by two, that's equal to 0.252 Moles of age feel this is again do the multiple ratios to find the massive H feel forms, However, I need to multiply by the Moeller massiveness. So this many moles multiplied by 36.46 grams of H feel in every one wall of age feel this is equal to 9.19 grams product.

Here were asked to consider the reaction of solid zinc with excess HCL reacting to form zinc chloride and H two gas. These in chloride and the HDL er a quiz. And so we're told that we result with 0.1 to 5 leaders of age to gas at STP. And so that's another way saying we have it at temperature to 73 Kelvin and a pressure of equal to equal to one atmosphere. And so we're basically asked how many moles of zinc did we start with for this to be the result? And so we need to figure out the moles of hydrogen gas that we have and because we have a 1 to 1 more ratio Haijun to sink, we're going to get the number of moles is sick when we should figure out from there the masses think that was reacting. So we're gonna use the ideal gas law solving for the number of moles. So an equals P V over our tea. I'm just gonna plug in the values that we have here. So the pressure we have one atmosphere would ignore the units for now 0.1 to 5 leaders over 0.8 to 1 as our gas constant and to 73 kelvin as our temperature. And so then the number of moves that we're going to get he's going to be equal to 5.57 times tense, a negative third malls of age to which is also able to the Moores of sick because we have a one so one ratio. And so since we have now the most of zinc, or ask to find the mask, we just need to multiply this number right here by the molecular weight of sink, which is 65.38 grams per mole. The moles will cancel out, and we're gonna get a final Masses Inc as 0.36 or grabs.


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