A 22.6 gram sample of krypton gas has a volume of 904 milliliters at a pressure of 2.71 atm. The temperature of the Kr gas sample is:

110.78 K

Explanation:

First we convert 22.6 g of krypton gas (Kr) to moles, using its molar mass:

Then we use the PV=nRT formula, where:

2.71 atm * 0.904 L = 0.270 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * T

And solve for T:

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."