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emmasim [6.3K]
2 years ago
5

Identify the balanced chemical equation that represents a combustion reaction. 2C 4H 10 + 13O 2 ⟶ 10H 2O + 8CO 2 C 4H 10 + 5O 2

⟶ 5H 2O + 4CO 2 CaCO 2 ⟶ Ca + CO 2 2CaCO 2 ⟶ 2Ca + CO 2
Chemistry
1 answer:
kati45 [8]2 years ago
7 0

Answer:

  2C₄H₁₀ + 13O₂ ⟶ 10H₂O + 8CO₂

Explanation:

  2C₄H₁₀ + 13O₂ ⟶ 10H₂O + 8CO₂  . . . . .  balanced combustion reaction

  C₄H₁₀ + 5O₂ ⟶ 5H₂O + 4CO₂  . . . . not balanced

The two reactions involving Ca are not combustion reactions.

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What is the pH of a 0.0042 M hydrochloric acid solution?
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E) 2.38

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The pH of any solution , helps to determine the acidic strength of the solution ,

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and ,

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pH is given as the negative log of the concentration of H⁺ ions ,

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pH = - log H⁺

From the question ,

the concentration of the solution is 0.0042 M , and being it a strong acid , dissociates completely to its respective ions ,

Therefore , the concentration of H⁺ = 0.0042 M .

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What mass of chromium would be produced from the reaction of 57.0 g of potassium with 199 g of chromium(II) bromide according to
fredd [130]

Answer:

Mass of Chromium produced = 37.91 grams

Explanation:

2K + CrBr₂  →  2KBr + Cr

2mole     1 mole                1 mole

mass of Potassium = 57.0 grams

molar mass of Potassium = 39.1 g/mol

no of moles of Potassium = 57.0 / 39.1 = 1.458 moles

mass of CrBr₂= 199 grams

molar mass of CrBr₂ = 211.8 gram/mole

no of moles of CrBr₂ = 199 / 211.8 = 0.939 mole

From chemical equation

1 mole of CrBr₂ = 2 moles of K

∴ 0.939 moles of CrBr₂ = ?

   ⇒ 0.939 x 2/1 = 1.878 moles of K

1.878 moles of K is needed, but there is 1.458 moles of K. So, Potassium is completed first during the reaction . Hence, Potassium is limiting reagent. and CrBr₂ is excess reagent .

From chemical equation

2 moles of K = 1 mole of Cr

∴ 1.458 moles of K = ?

   ⇒ 1.458 x 1/ 2 = 0.729 moles of Cr

no of moles of Cr formed = 0.729 moles

molar mass of Cr = 52.0 g/mol

mass of one mole of Cr = 52.0 grams

mass of 0.729 moles of Cr = 52.0 x 0.729 = 37.908 grams

mass of Chromium produced = 37.91 grams

6 0
3 years ago
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