Barium reacts with water to produce barium hydroxide and hydrogen gas. How many moles of barium hydroxide are produced when 250.0 mL of water is consumed? (NOTE: water is in the liquid state. Assume the density of water is 1.00 g/mL) What is the total number of moles of ions from barium hydroxide produced in this reaction?

Given that the molar mass of nano3  is 85.00  g/mol, what mass of nano3  is needed to make 4.50  l of a 1.50  m nano3solution? use  .6.75 g18.9 g255 g574 g

Why doesn't heat added to water make the tempature rise above 100c

Consider the following reaction at equilibrium. 2co2 (g) 2co (g) + o2 (g) h° = -514 kj le châtelier's principle predicts that the equilibrium partial pressure of co (g) can be maximized by carrying out the reaction a. at high temperature and high pressure b. at high temperature and low pressure c. at low temperature and low pressure d. at low temperature and high pressure e. in the presence of solid carbon