5 when copper metal is added to nitric acid the reaction...

5. When copper metal is added to nitric acid, the reaction given below takes place Cu (s) + 4 HNO3 (aq) → Cu(NO3)2 (aq) + 2 H2O (l) + 2 NO2 (g) Calculate the volume (in liters) of NO2 gas collected over water at 25.0 °C when 2.01 g of copper is added to excess nitric acid if the total pressure is 726.0 mm Hg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg

Transcript

00:01 Hi, so we are to calculate the volume of no2 gas that is collected over water at the given pressure and also pressure and we're given with the initial amount of copper.

00:14 So first we have to calculate the number of moles of no2 produced from the given amount of copper.

00:22 So we have 2 .01 grams of copper and then we will divide the molar mass of copper from the predict table that's 63 .55.

00:31 Grams so we have moles of copper in the numerator and take the stoichiometric ratio from the balance equation you can see that for everyone mole of copper reacted it will produce two moles of and 02 so we could cancel grams of copper moles of copper then calculating this 2 .01 times 2 divided by 603 .55 is 0 .06 3266 this is molose of n02.

01:05 Now to solve for the volume, we will use the ideal gas equation.

01:09 Pv is equivalent to nrt.

01:12 But we need to calculate first the pressure because this is collected over water.

01:17 So we'll subtract the vapor pressure of water from the total pressure.

01:22 Let's just do it here.

01:25 Total pressure is 726 mmhg and the vapor pressure of water at the given temperature is 23 .8 mhmhg.

01:34 So pressure would be 726 minus 203 .8.

01:39 That's 702 .2 m .hg.

01:44 So let's rearrange the formula.

01:45 The ideal gas law equation to solve for v will have nrt over the pressure.

01:51 Now plug in the values here...