The chemical equation for the manufacture of ammonia is N 2 ( g ) + 3 H 2 ( g ) → 2 NH 3 ( g ) Calculate the amount of H 2 required to react with 28 g of N 2 completely. [Molecular mass of N 2 = 28 u , H 2 = 2 u ]

The amount of H 2 required to react with 28 g of N 2 completely is: 28 g N 2 is equal to 1 mol N 2 1 mol of N 2 requires 3 mol of H 2 Hence, mass of H 2 = 3 × 2 g = 6 g

The chemical equation for the manufacture of ammonia is N 2 ( g ) + 3 H 2 ( g ) → 2 NH 3 ( g ) What will be the volume of NH 3 formed at STP, if 22 . 4 L of N 2 is completely reacted?

22 . 4 L N 2 is equal to 1 mol N 2 1 mol N 2 undergoes reaction to produce 2 mol NH 3 . Therefore, the volume of NH 3 formed at STP = 2 × 22 . 4 = 44 . 8 L .

The molecular mass of methane ( CH 4 ) is 16 u . . What is the mass of 5 × 6 . 022 × 10 23 CH 4 molecules?

The molar mass of methane ( CH 4 ) is = 16 g Number of methane molecules = 5 × 6 . 022 × 10 23 1 mole of methane molecules = 6 . 022 × 10 23 So, number of moles of methane = 5 × 6 . 022 × 10 23 6 . 022 × 10 23 = 5 Moles = 5 Molar mass of methane = 16 g Mass = moles × molar mass Mass of 5 moles of methane molecules = 5 × 16 = 80 g .

Embibe Experts Solutions for Chapter: Gas Laws and Mole Concept, Exercise 1: Kerala Board-2018

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Embibe Experts Chemistry Solutions for Exercise - Embibe Experts Solutions for Chapter: Gas Laws and Mole Concept, Exercise 1: Kerala Board-2018

Attempt the free practice questions on Chapter 2: Gas Laws and Mole Concept, Exercise 1: Kerala Board-2018 with hints and solutions to strengthen your understanding. EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY solutions are prepared by Experienced Embibe Experts.