A calorimeter contains 30.0 mL of water at 13.0 °C. When 1.30 g of X (a substance
with a molar mass of 46.0 g/mol) is
added, it dissolves via the reaction
X(s) + H2O(1) X(aq)
and the temperature of the solution
increases to 28.5 °C.
Calculate the enthalpy change, AH, for
this reaction per mole of X.
Assume that the specific heat of the
resulting solution is equal to that of water
[4.18 J/(g• °C)], that density of water is
1.00 g/mL, and that no heat is lost to the
calorimeter itself, nor to the surroundings.

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the term hydride is commonly named after binary compounds that hydrogen forms with other elements of the periodic table. hydride compounds in general form with almost any element, except a few noble gases. the trends and properties vary according to the type of intermolecular force that bonds the elements together, the temperature, its molecular masses, and other components. hydrides are classified into three major groups, depending on what elements the hydrogen bonds to. the three major groups are covalent, ionic, and metallic hydrides. formally, hydride is known as the negative ion of a hydrogen, h-, also called a hydride ion. because of this negative charge, hydrides have reducing, or basic properties. its special characteristics will be further discussed.

explanation: