Five samples of krypton gas are described in the table below. Rank the samples in order of increasing average kinetic energy of the atoms in them. That is, select "1" next to the sample in which the krypton atoms have the lowest average kinetic energy. Select "2" next to the sample in which the krypton atoms have the next lowest average kinetic energy, and so on. amount 2.2 mol 1.7 mol 2.0 mol 1.4 mol 1.9 mol sample pressure 1.4 atm 1.6 atm 2.6 atm 1.5 atm 3.0 atm temperature -9. °℃ -1. °C -18. °C -33. °C 5. °C average kinetic energy of atoms in sample Ⓒ Ⓒ «

please see the attached image

When the two atoms are approaching each other, which statement is true about the potential energy (PE) of the system and the kinetic energy (KE) of the atom? A. Potential energy decreases and kinetic energy increase  b. Potential energy increase and kinetic energy decrease  c. They both remain constant

3. Suppose the 25.0 g of the following substances all initially at 27.0 °C absorb 2.35 kJ of energy. What is the final temperature of each? A) gold   B) silver   C) Aluminum   D) Water.  I also needed to look up specific heat values.

The units for the answer is KJ/mol. But this answer says joules. why is that?

The First Law of Thermodynamics, known as Conservation of Energy, states that when energy is transformed, the total stays the same. Describe TWO examples of the first law, one involving living organisms and one not involving living organisms.

Hess's Law Prelab Questions Name Section 1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? of aola) Goules)

Use data from table (Figure 1), the figure (Figure 2) and the figure (Figure 3) to calculate the lattice energy of RbCl

Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ  Reaction 2: 2OF2(g)⟶O2(g)+2 F2(g)ΔH=−49.4 kJ  Reaction 3: N2(g)+2O2(g)⟶2NO2(g)ΔH=+66.4 kJ    Use Reaction 2.   How much energy (in kJ) is released when 79.0 g of oxygen difluoride decomposes?

using the equations provided, please help me figure out which of them goes to which problems which have also been provided