(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.