When nitrogen dioxide (NO2) from car exhaust combines w/ water in the air it forms nitric acid (HNO3), which causes acid rain, and nitrogen monoxide. 3NO2(g)+ H2O(L)----->2HNO3(aq)+ N(g) a.How many molecules of NO2 are needed to react with 0.250 mole H2O?

b.How many grams of CO2 could be produced from the complete reaction of the acetylene in part a?

sorry wrong info

To determine the number of molecules of NO2 needed to react with 0.250 mole of H2O, you need to use the balanced chemical equation. The coefficients in the balanced equation represent the mole ratios between the reactants and products.

The balanced equation for the reaction is:
3NO2(g) + H2O(L) → 2HNO3(aq) + N(g)

a) To find the number of molecules of NO2 needed, you need to use the mole ratio between NO2 and H2O. From the balanced equation, you can see that for every 1 mole of H2O, 3 moles of NO2 are needed. Therefore, you can set up the following ratio:

3 moles NO2 / 1 mole H2O

Next, you need to convert the moles of H2O given to moles of NO2 using the ratio. Since you have 0.250 mole of H2O, you can multiply it by the ratio:

0.250 mole H2O * (3 moles NO2 / 1 mole H2O) = 0.750 mole NO2

Now, you can convert from moles to molecules. Avogadro's number tells us that 1 mole of any substance contains 6.022 x 10^23 molecules. Therefore, you can use Avogadro's number to convert from moles to molecules:

0.750 mole NO2 * (6.022 x 10^23 molecules / 1 mole) = 4.5165 x 10^23 molecules NO2

So, approximately 4.5165 x 10^23 molecules of NO2 are needed to react with 0.250 mole of H2O.

b) The question asks how many grams of CO2 could be produced from the complete reaction of the acetylene in part a. However, the given balanced equation does not contain any acetylene (C2H2). Therefore, it seems there might be a mistake or missing information in the question.