(temperature is negative) how many liters of no2 (at stp) can be produced from 149 grams of cu reacting with concentrated nitric acid, hno3 (aq)?

(the equation is balanced)

cu + 4 hno3 ⇒ cu(no3) 2 + 2 h2o + 2 no2

63.55, 63.02, 187.57, 18.02, 46.01
^ g/mol

Explanation:

We will need a balanced chemical equation with molar masses and volumes, so, let's gather all the information in one place.

MV/L:                                                                     22.71

M_r:         63.55

                  Cu + 4HNO₃ ⟶ Cu(NO₃)₂ + 2H₂O + 2NO₂

m/g:           149

(a) Moles of Cu

(b) Moles of NO₂

The molar ratio is 2 mol NO₂:1 mol Cu

(c) Volume of NO₂

The volume of 1 mol of an ideal gas at STP (0 °C and 1 bar) is 22.71 L.

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.