Acetic acid (CH3COOH) reacts with water to form the acetate ion and the hydronium ion: Upper C upper H subscript c upper C upper O upper o upper H (a q) plus upper H subscript 2 upper o (l) double arrow upper C upper H subscript 3 upper C upper o upper O superscript minus (a q) plus upper H subscript 3 upper o superscript plus (a q).

At equilibrium, the concentration of CH3COOH is 2.0 × 10–1 M, the concentration of CH3COO– is
1.9 × 10–3 M, and the concentration of H3O+ is 1.9 × 10–3 M. What is the value of Keq for this reaction?

1.8 × 10–5

5.5 × 104

9.5 × 10–3

1.1 × 102

A48 g piece of ice at 0.0 ∘c is added to a sample of water at 7.4 ∘c. all of the ice melts and the temperature of the water decreases to 0.0 ∘c. how many grams of water were in the sample?

Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, pbutane, alone. to do this, consult a reference and record the partial pressure of the water vapor, pwater, at the temperature you recorded. use the following formula to compute the partial pressure of the butane. pbutane = atmosphere - pwater use the following combined gas law formula and compute the volume that the butane sample will occupy at stp. (hint: convert both temperatures to kelvin.) pbutane x voriginal = pstandard x vfinal troom tstandard use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. grams of butane you used “x” grams of butane ml of butane corrected to stp = 22,400 ml compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table. compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula: % error = measured value - accepted value x 100 accepted value use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. need asap

At 20°c, a sample of h2o liquid and a sample of co2 gas each have the same average kinetic energy. why is one a liquid and the other a gas at this temperature?