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Galina-37 [17]
3 years ago
10

A seashell, composed largely of calcium carbonate, is placed in a solution of HCl. As a result, 1700 mL of dry CO2 gas at STP is

produced. The other products are CaCl2 and H2O. Based on the information, how many grams of CaCO3 are consumed in the reaction? The density of CO2 at STP = 1.997 g/L (STP stands for standard temperature and pressure).
Chemistry
1 answer:
Nadusha1986 [10]3 years ago
5 0

Answer:

7.7g CaCo3

Explanation:

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kotykmax [81]

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NikAS [45]

Answer:

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Explanation:

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7 0
3 years ago
The equilibrium constant for the chemical equation N2(g) + 3H2(g) ⇌ 2NH3(g) and Kp=0.174 at 243°C. Calculate the value of Kc for
Mashcka [7]

Answer:

The Kc of this reaction is 311.97

Explanation:

Step 1: Data given

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Step 2: The balanced equation

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Step 3: Calculate Kc

Kp = Kc *(RT)^Δn

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⇒ with Kc = TO BE DETERMINED

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0.174 = Kc (0.08206*516)^-2

Kc = 311.97

The Kc of this reaction is 311.97

3 0
3 years ago
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umka21 [38]

Answer:

25 mph

Explanation:

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2 years ago
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8 0
3 years ago
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