Pure water is used to dilute $192l{b}_m$ of a sulfuric acid stream that has an initial mass fraction of $H_{2}S{O}_4$ equal to $0\mathrm{.}85$ in order to

produce a diluted acid with an $H_{2}S{O}_4$ mass fraction of $0\mathrm{.}45.$ The temperature of the water is $40F$ and that of the concentrated acid is

$77F.$

An enthalpy$-$composition diagram for the system is shown below.

Enthalpy$-$concentration chart for $H_{2}S{O}_4-H_{2}O.($Redrawn from the data of W$.$ D$.$ Ross, Chem. Eng. Progr., $43$:$314,1952.)$

Heat Liberated

Check the specific enthalpies of the hot product and the chilled product.

How much heat would have to be removed from the system for the diluted product to emerge at $100F?$

$|Q|=$

Btu

Hint

Assistance Used

Use three quantities: the mass of the product, the specific enthalpy of the hot product, and the specific enthalpy of the chilled

product.