$$Ca(s)+2H_{2}O(l)\rightarrow Ca(OH)_{2}(aq)+H_{2}(g)$$

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Reason
The reaction of calcium with water is less violent. The heat evolved is not sufficient for the hydrogen to catch fire. the bubbles of hydrogen gas formed stick to the surface of the water calcium
Assertion
$$Ca(s) + 2H_2O(l) \rightarrow Ca(OH)_2(aq) + H_2(g)$$
calcium floats over water during the reaction with water
$$Ca(s) + 2H_2O(l) \rightarrow Ca(OH)_2(aq) + H_2(g)$$
calcium floats over water during the reaction with water

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Identify X in the following reaction:

C a (O H)_{2} (a q) + 2 X \to C a C l_{2} (a q) + 2 H_{2} O (l)

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H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 H_{2} O (l); Δ H = - 86 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) . . . . . . . . . k J (\pm ?)

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H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 H_{2} O (l); Δ H = - 286 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) . . . . . . . . . k J (\pm ?)

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Calculate the value of

Δ H (k J)

for the following reaction using the listed thermochemical equations

2 C (s) + H_{2} (g) \to C_{2} H_{2} (g)

2 C_{2} H_{2} (g) + 5 O_{2} (g) ⟶ 4 C O_{2} (g) + 2 H_{2} O (l)

;

Δ H^{o} = - 2600 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g)

;

Δ H^{o} = - 390 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l)

;

Δ H^{o} = - 572 k J

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