Consider an experimental run at 273 K where the initial number of moles (n1) is actually 1.00 mol, and the final number of moles (n2) is 2.00 mol. Use the simulation to find the volume (V1) of 1.00 mol of helium at 273 K, and calculate the final volume (V2). Express the volume to three significant figures, and include the appropriate units.

The volume of 1.00 mol of helium at 273 K is 22.4 L and the final volume is 44.8 L.

Explanation:

Given: = 273 K,   = 1.00 mol

= 273 K,         = 2.00 mol

At the standard pressure, 1 atm the value of and is calculated as follows.

Similarly,

Thus, we can conclude that the volume of 1.00 mol of helium at 273 K is 22.4 L and the final volume is 44.8 L.

here are some of the ways in which chemical and nuclear reactions differ.

explanation:

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: