Heat of combustion of A(s) is -10 k Cal mole-1 and that of B(s) is -15 k Cal mole-1 , mixture containing 3 moles A(s) and x moles B(s) on combustion released 105 K cal of heat. What is the value of x …….?(During combustion solid A forms AO2 and solid B forms BO2)

First, let's calculate the total heat released by the combustion of 3 moles of A(s). The heat of combustion of A(s) is -10 k Cal mole-1, so the heat released by the combustion of 3 moles of A(s) is:

3 moles A(s) * (-10 k Cal mole-1) = -30 k Cal

Next, let's calculate the total heat released by the combustion of x moles of B(s). The heat of combustion of B(s) is -15 k Cal mole-1, so the heat released by the combustion of x moles of B(s) is:

x moles B(s) * (-15 k Cal mole-1) = -15x k Cal

The total heat released by the combustion of the mixture is given as 105 k Cal. Therefore, we can set up the equation:

-30 k Cal + (-15x k Cal) = 105 k Cal

Simplifying the equation, we have:

-30 k Cal - 15x k Cal = 105 k Cal

Combining like terms, we get:

-45x k Cal = 105 k Cal

Dividing both sides of the equation by -45 k Cal, we find:

x = -105 k Cal / -45 k Cal

Simplifying further, we have:

x = 2.33

Therefore, the value of x is approximately 2.33 moles.