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Standard VIII

Chemistry

Shortcut-Balancing

Write the bal...

Question

Write the balanced chemical equation for the given reaction:
Crystalline C $_{6}$ H $_{12}$ O $_{6}$ is burnt in the present of oxygen to form carbon dioxide and water vapour.

_{6}

_{12}

_{6}

(s) + 3O

_{2}

(g)

\to

6CO

_{2}

(g) + 6H

_{2}

O(g)

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_{6}

_{12}

_{6}

(s) + 6O

_{2}

(g)

\to

6CO

_{2}

(g) + 6H

_{2}

O(g)

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_{6}

_{12}

_{6}

(s) + 6O

_{2}

(g)

\to

3CO

_{2}

(g) + 3H

_{2}

O(g)

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_{6}

_{12}

_{6}

(s) + 6O

_{2}

(g)

\to

6CO

_{2}

(g) + 3H

_{2}

O(g)

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Solution

The correct option is A C $_{6}$ H $_{12}$ O $_{6}$ (s) + 6O $_{2}$ (g) $\to$ 6CO $_{2}$ (g) + 6H $_{2}$ O(g)
When one molecule of glucose is burnt in presence of excess oxygen then it is converted to 6 molecules of carbon dioxide gas and 6 molecules of water vapor. The balanced chemical equation is $C_{6} H_{12} O_{6} (s) + 6 O_{2} (g) \to 6 C O_{2} + 6 H_{2} O$ . So the correct option is B

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Similar questions

6CO

_{2}

+ 6H

_{2}

\to

_{6}

_{12}

_{6}

+ 6O

_{2}

The site of this process is:

Consider the reactions:

(a) 6 CO₂(g) + 6H₂O(l) → C₆ H₁₂ O₆(aq) + 6O₂(g)

(b) O₃(g) + H₂O₂(l) → H₂O(l) + 2O₂(g)

Why it is more appropriate to write these reactions as:

(a) 6CO₂(g) + 12H₂O(l) → C₆ H₁₂ O₆(aq) + 6H₂O(l) + 6O₂(g)

(b) O₃(g) + H₂O₂ (l) → H₂O(l) + O₂(g) + O₂(g)

Also suggest a technique to investigate the path of the above (a) and (b) redox

reactions.

Q. At

27 C

the reaction,

C_{6} {H_{6}}_{(l)} + \frac{15}{2} {O_{2}}_{(g)} \to {6 C O}_{2}_{(g)} + {{3 H}_{2} O}_{(l)}

proceeds spontaneously because the magnitude of?

Consider the reactions:
$6 C O_{2} (g) + 6 H_{2} O (l) \to C_{6} H_{12} O 6 (a q) + 6 O_{2} (g)$
Why it is more appropriate to write these reactions as:
$6 C O_{2} (g) + 12 H_{2} O (l) \to C_{6} H_{12} O_{6} (a q) + 6 H_{2} O (l) + 6 O_{2} (g)$
Also suggest a technique to investigate the path of the above (a) and (b) redox reactions.

$O_{3} (g) + H_{2} O_{2} (l) \to H_{2} O (l) + 2 O_{2} (g)$
Why it is more appropriate to write these reactions as:
$O_{3} (g) + H_{2} O_{2} (l) \to H_{2} O (l) + O_{2} (g) + O_{2} (g)$
Also suggest a technique to investigate the path of the above (a) and (b) redox reactions.

How many of these reactions are homogeneously catalyzed? ___

(i) $2 S O 2 (g) + O_{2} (g) N O (g) - --- \to 2 S O_{3} (g)$

(ii) $C_{12} H_{22} O_{11} (a q .) + H_{2} O (ℓ) H_{2} S O_{4} (ℓ) - ----- \to C_{6} H_{12} O_{6} G l u c o s e (a q .) + C_{6} H_{12} O_{6} F r u c t o s e (a q .)$

(iii) $2 S O_{3} (g) + O_{2} (g) P t (s) - -- \to 2 S O_{3} (g)$

(iv) $N_{2} (g) + 3 H_{2} (g) F e (s) - -- \to 2 N H_{3} (g)$

(v) $4 N H_{3} (g) + 5 O_{2} (g) P t (s) - -- \to 4 N O (g) + 6 H_{2} O (g)$

(vi) $C H_{3} C O O C H_{3} (ℓ) H C l (ℓ) - --- \to C H_{3} C O O H (a q .)$

(vii) Vegetable oils $(ℓ) + H_{2} (g) N i (s) - -- \to$ Vegetable ghee

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Write the balanced chemical equation for the given reaction:Crystalline C6H12O6 is burnt in the present of oxygen to form carbon dioxide and water vapour.

Write the balanced chemical equation for the given reaction:
Crystalline C $_{6}$ H $_{12}$ O $_{6}$ is burnt in the present of oxygen to form carbon dioxide and water vapour.