When 1.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C. If the specific heat of the solution is 4.18 J/(g ∙ °C), calculate for the reaction, as written. Ba(s) + 2 H2O(l) → Ba(OH)2(aq) + H2(g)

The amount of heat is 431.12 kJ/mol.

Explanation:

Given that,

Mass of Ba = 1.50 g

Mass of water = 100.0 g

Initial temperature = 22.00°C

Final temperature = 33.10°C

The reaction is,

We need  to calculate the heat

Using formula of heat

Where, m = mass

s = specific heat

temperature

Put the value into the formula

We need to calculate the amount of heat per mole

Using formula of energy per mole

Put the value into the formula

Hence, The amount of heat is 431.12 kJ/mol.

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explanation:

the awnser is group 12