How many kilograms of nh3 are needed to produce 1.90x10^5 of (nh4)2so4? answer in scientific notation

Molar mass :

NH₃ = 17.0 g/mol

(NH₄)₂SO₄ = 132 g/mol

2 NH₃ + H₂SO₄ = (NH₄)₂SO₄

2 x 17 g NH₃ 132 g  (NH₄)₂SO₄
( mass NH₃) 1.90 x 10⁵  (NH₄)₂SO₄

( mass NH₃) = (1.90 x 10⁵) x 2 x 17 / 132

( mass NH₃) = 6460000 / 132

( mass NH₃) = 48939.39 g

in kg :

48939.39 / 1000 = 48.93 kg = 4.893 x 10¹ kg

hope this helps!

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The activity series is shown in the attached picture. if the element is below the other, then you can displace the other. following the activity series as a guide, the reactions are as follows: nickel and aluminum chloride3 ni + 2 alcl₃  → 3 nicl₂ + 2 albarium and copper bromideba + cubr  →  no reaction because cu is less oxidizable than bapotassium nitrate and aluminum3 kno₃ + al  → al(no₃)₃ + 3 ksodium phosphate and zincnaso₄ + zn  → znso₄ + na