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vlada-n [284]
2 years ago
7

At a certain temperature, iron (II) oxide, FeO, can react with carbon monoxide, CO, to form elemental iron, Fe, and carbon dioxi

de, CO2. The value of Kp at that temperature is 0.242. What is the pressure of CO2 at equilibrium if a sample of FeO was initially in a container with CO at a pressure of 0.95 atm? The chemical reaction involved in this process is: FeO(s) + CO(g) ⟷ Fe(s) + CO2(
Chemistry
1 answer:
barxatty [35]2 years ago
7 0

Answer:

The pressure of CO2 at the equilibriumis 0.185 atm

Explanation:

Step 1: Data given

The value of Kp at that temperature is 0.242

FeO was initially in a container with CO at a pressure of 0.95 atm

Step 2: The balanceequation

FeO(s) + CO(g) ⟷ Fe(s) + CO2(g)

Step 3:The initial pressure

pCO = 0.95 atm

pCO2 = 0 atm

Step 4: The pressure at the equilibrium

pCO = 0.95 - x atm

pCO2 = X atm

Step 5: Calculate Kp

Kp = pCO2 / pCO

0.242 = X / (0.95 - X)

X = 0.185

pCO = 0.95 - 0.185 =  0.765 atm

pCO2 = 0.185 atm

The pressure of CO2 at the equilibriumis 0.185 atm

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What is the relationship between producers and consumers in a food chain a producers eat consumers b consumers eat producers c p
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b consumers eat producers

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What mass of water (in grams) is produced by the reaction of 23.0 g of SiO2?
nikitadnepr [17]

The mass of water produced by the reaction of the 23 g of SiO_2  is 13.8 g.

The given chemical reaction;

4Hf (g)  \ + \ SiO_2 (s) \ --> \ SiF_4(g) \ + \ 2H_2O(l)

In the given compound above, we can deduce the following;

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60 g of SiO_2  --------- 36 g of water

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Thus, the mass of water produced by the reaction of the 23 g of SiO_2  is 13.8 g.

  • <em>"Your question is not complete, it seems to be missing the following information";</em>

In the reaction of the given compound, 4Hf (g)  \ + \ SiO_2 (s) \ --> \ SiF_4(g) \ + \ 2H_2O(l), what mass of water (in grams) is produced by the reaction of 23.0 g of SiO2?

Learn more here:brainly.com/question/13644576

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