Register to reply

Stoichiometry: yield of reaction between hydrochloric acid and calcium carbonate

Share this thread:
pc2-brazil
#1
Nov15-08, 07:40 AM
P: 205
Thank you in advance for the correction of the resolution.

1. The problem statement, all variables and given/known data

By reacting 225 g of hydrochloric acid with 300 g of calcium carbonate with 80% of purity, 34 L (litres) of gas were obtained, measured at 37oC and a pression of 0.82 atm. What is the yield of this reaction and what mass of calcium carbonate reacted? (Remember that H2CO3, in water, decomposes as water and CO2)

[tex]2HCl_{(aq)} + CaCO_3_{(s)} \rightarrow CaCl_2_{(s)} + H_2CO_3_{(aq)}[/tex]

R = 0.082 (atm*L)/(mol*K).

2. Relevant equations

[tex]PV = nRT[/tex]

3. The attempt at a solution

[tex]2HCl_{(aq)} + CaCO_3_{(s)} \rightarrow CaCl_2_{(s)} + H_2O_{(aq)} + CO_2_{(g)}[/tex]
Molecular masses: 2 HCl = 2(36.5) = 73 g; 1CaCO3 = 100 g.
Assuming that the expression "with 80% of purity" refers to calcium carbonate (we are not sure):
The molar relation in order to know the limiting reagent (but the purity of the calcium carbonate is 80%, so 300 g * 80% = 240 g):
[tex]1 mol HCl \rightarrow 1 mol CaCO_3[/tex]
[tex]73 g \rightarrow 100g[/tex]
[tex]x \rightarrow 300 \times 0.8[/tex]
x = 175.2 g of HCl. Smaller than the available quantity, 225 g, thus it is in excess. The limiting reagent is CaCO3.
Now, the molar relation between calcium carbonate and the gas, CO2, in order to find how many litres of the gas (y) are produced with 100% yield.
But first, to find the molar volume:
37oC = 37 + 273 = 310 K.
[tex]PV_m = nRT \rightarrow 0.82V_m = 0.082 \times 310 \rightarrow V_m = 31 L[/tex]
[tex]1 mol CaCO_3 \rightarrow 1 mol CO_2[/tex]
[tex]100 g \rightarrow 31L[/tex]
[tex]240 g \rightarrow y[/tex]
y = (31 * 240) / 100
y = 74.4 L.
What is the yield of this reaction?
Since the volume of gas produced with the current yield is 34 L, the yield (R) is:
[tex]R = \frac{34}{74.4}[/tex]
R = 45.6%.
What mass of calcium carbonate reacted?
It was already calculated: 240 g.
Phys.Org News Partner Science news on Phys.org
'Office life' of bacteria may be their weak spot
Lunar explorers will walk at higher speeds than thought
Philips introduces BlueTouch, PulseRelief control for pain relief
Borek
#2
Nov15-08, 08:48 AM
Admin
Borek's Avatar
P: 23,719
Could be the final question (about the mass of carbonate that reacted) asks how much carbonate reacted to give 34L of CO2 assuming 100% yield. It is not clear to me.
pc2-brazil
#3
Nov15-08, 09:08 AM
P: 205
Quote Quote by Borek View Post
Could be the final question (about the mass of carbonate that reacted) asks how much carbonate reacted to give 34L of CO2 assuming 100% yield. It is not clear to me.
Thank you for the response.
If the calcium carbonate is the limiting reagent, then the mass that reacted is simply the quantity given in the enunciation (considering the purity), right? Unfortunately, we would have to wait until Friday to ask exactly what the teacher meant.
It is strange that CaCO3 was the limiting reagent. If it was the one in excess, then the last question would appear more appropriate, because then we would have to find how many of the CaCO3 was actually used...
Anyway, is the yield of 45,6% right?

pc2-brazil
#4
Nov29-08, 07:03 AM
P: 205
Stoichiometry: yield of reaction between hydrochloric acid and calcium carbonate

We confirmed it with the teacher: 240 g is the right answer.


Register to reply

Related Discussions
Hydrochloric acid Chemistry 14
Stoichiometry: finding the yield in reaction of sodium azide with iron oxide Biology, Chemistry & Other Homework 3
Calcium Carbonate CaCO3 Biology, Chemistry & Other Homework 2
Stoichiometry, Part II (and Percentage Yield) Biology, Chemistry & Other Homework 4
Hydrochloric Acid Chemistry 1