Oh, no! you just spilled 85.00 ml of 1.500 m sulfuric acid on your lab bench and need to clean it up immediately! right next to you there is a small jar labeled "15.00 g sodium bicarbonate". will this be enough sodium bicarbonate to neutralize the spilled sulfuric acid? show your work and state all reasoning!

Explanation:

We will balance equation which describes the reaction between sulfuric acid and sodium bicarbonate: as follows.

Next we will calculate how many moles of are present in 85.00 mL of 1.500 M sulfuric acid.

As,       Molarity =

            1.500 M =

                    n = 0.1275 mol

Now set up and solve a stoichiometric conversion from moles of  to grams of . As, the molar mass of is 84.01 g/mol.

                 = 21.42 g

So unfortunately, 15.00 grams of sodium bicarbonate will "not" be sufficient to completely neutralize the acid. You would need an additional 6.42 grams to complete the task.

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

hurricanes form when warm, moist air from the ocean surface quickly rises into the atmosphere and forms storm clouds and rain. when the clouds are formed, heat is released which warms the cool air in the upper regions of the atmosphere so that the cycle can continue. which two phases of the water cycle are repeated in this process?