Question

Using the Haber process, represented by the balanced chemical equation below, 296 L of ammonia are made. How many litres of nitrogen were needed, assuming excess of hydrogen was present to make this much ammonia? All gas measurements are made at the same temperature and pressure. N2(g) + 3 H2(g) → 2 NH3(g),

Name: using the haber process represented by the balanced chemical equation below 296 l of ammonia are made how many litres of nitrogen were needed assuming excess of hydrogen was present to make 86118
Uploaded: 2022-06-09T02:33:52-08:00
Duration: 3 min 4 s
Channel: Sri K
Description: using the haber process represented by the balanced chemical equation below 296 l of ammonia are made how many litres of nitrogen were needed assuming excess of hydrogen was present to make 86118

          Using the Haber process, represented by the balanced chemical
equation below, 296 L of ammonia are made. How many litres of
nitrogen were needed, assuming excess of hydrogen was present to
make this much ammonia? All gas measurements are made at the same
temperature and pressure. N2(g) + 3 H2(g) → 2 NH3(g),

Added by Guillermo P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

06/09/2022

Step 1

Given that 1 mole of gas at standard conditions is equal to 22.4 L, we can calculate the moles of ammonia produced by dividing 296 L by 22.4 L/mol. Moles of NH3 = 296 L / 22.4 L/mol = 13.2 mol Show more…

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Using the Haber process, represented by the balanced chemical equation below, 296 L of ammonia are made. How many litres of nitrogen were needed, assuming excess of hydrogen was present to make this much ammonia? All gas measurements are made at the same temperature and pressure. N2(g) + 3 H2(g) → 2 NH3(g),