Consider 2.00 mol of an ideal gas with a constant‑volume molar specific heat of 12.5 J/(mol·K), an initial temperature of 22.8 ∘C, and an initial pressure of 5.210×10^4 Pa. The state of the gas is then changed to a final temperature of 44.1 ∘C and a final pressure of 3.090×10^4 Pa. What is the change in the entropy Δ of the gas during this process? The gas constant is 8.31 J/(mol·K).

I keep getting 10.7 J/K but it is wrong. Can someone explain?

Which of the following compounds does not contain molecules? question 2 options: co2 h2 nacl h2o

Base your answer on the information below and on your knowledge of chemistry. nitrogen dioxide, no2, is a dark brown gas that is used to make nitric acid and to bleach flour. nitrogen dioxide has a boiling point of 294 k at 101.3 kpa. in a rigid cylinder with a movable piston, nitrogen dioxide can be in equilibrium with colorless dinitrogen tetroxide, n2o4. this equilibrium is represented by the equation below. 2no2(g) n2o4(g) + 58kj at standard pressure, compare the strength of intermolecular forces in no2(g) to the strength of intermolecular forces in n2(g).

If 90.0 grams of ethane reacted with excess chlorine,how many grams of dicarbon hexachloride would form