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My name is Ann [436]
3 years ago
15

Aqueous carbonic acid H2CL3decomposes into carbon dioxide gas and liquid water . Write a balanced chemical equation for this rea

ction.
Chemistry
2 answers:
den301095 [7]3 years ago
7 0
H2co3 ___> CO2 + H2o
quester [9]3 years ago
7 0

Answer:

H2CO3(aq) ⇆ H2O(l) + CO2(g)

Explanation:

Step 1: Data given

Aqueous carbonic acid = H2CO3

H2CO3 decomposes into CO2 and H2O

Step 2: Balancing the equation

H2CO3(aq) ⇆ H2O(l) + CO2(g)

We do not have to change anything in this reaction since it's already balanced.

We have 2x H on both sides ( 2x in H2CO3 and 2x in H2O)

We have 1x C on both sides (1x in H2CO3 and 1x in CO2)

We have 3x O on both sides (3x in H2CO3 and 1x in H2O, 2x in CO2)

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IgorLugansk [536]
If we were to make room for errors, there should really be no limiting reagent because practically all of both Nitrogen and Hydrogen is used up during this reaction. If this values were actually exact, then Nitrogen would be the limiting reagent, but a very very little amount of Nitogen is needed for all the Hydrogen to react.

We solve this problem by first writing the equation
N2 + 3H2 = 2NH3
N2 = 14g*2 = 28g, 3H2 = 3(1*2) = 6g
so 28g of Nitrogen needs 6g of Hydrogen for this reaction. Thus if we had 10.67g of Hydrogen in the reaction, 6g*49.84g/28g of hydrogen is needed to react = 10.68g of Hydrogen, but since we have 10.7g of it thus it is excess and thus the limiting reagent has to be Nitrogen, but notice that 10.68g and 10.7g are practically the same, so there might actually not be a limiting reagent. Using the other value(10.7), the amount of Nitrogen required would be 10.7g*28g/6g = 49.93, and since this is slightly more than the 49.84g we have, this confirms that Nitrogen is the limiting reagent. But note still that since this values are really close, there is a possibility that there is neither a limiting nor an excess reagent
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3 years ago
an ------ model with dark bands representing energy levels shows where an atoms electrons are most likely to be.
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How many kilocalories of heat are released when 75 g of steam at 100 degrees Celsius is converted to ice at 0 degrees Celsius?
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Answer:

∴ Q = -7.52kCal

Explanation:

Using the formula for specific heat capacity:

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where ΔT = change in temperature (final - initial)  = (0 - 100)°C = -100°C

m = mass (g) = 75g

c = specific heat capacity = 4.2 J/g°C in water

⇒ Q = 75 × 4.2 × -100

= -31,500J

But 1J - 0.000239kCal

<u>∴ Q = -7.52kCal</u>

<u />

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