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 .

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 .

Select from the box, the correct gas law related to the given situation. Boyle's law, Charles law, Avagadro's law The size of the air bubble rising from the bottom of an aquarium increases

At constant temperature V α 1 P (Boyle's law) since as the air bubble rises upward, pressure decreases, then from above law volume of the bubble increases i.e. its size increases. The size of an air bubble rising up in water increases. When an air bubble rises in water, the pressure acting on the air bubble decreases. As the pressure exerted by water is directly proportional to the depth of water, as the depth of water increases in a water body, the pressure increases linearly.

Select from the box, the correct gas law related to the given situation. Boyle's law, Charles law, Avagadro's law An inflated balloon kept at sunlight bursts after some time.

It obeys Charle's law. It sates that When the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be in direct proportion. The kinetic energy of the gases increase with the increase in temperature. When the balloon is kept in the sun, due to the Sun's heat, the kinetic energy of gaseous particles inside the balloon also gets increased and the balloon expands. This will increase the pressure on the walls of the balloon. It continues to expand and comes to a stage when the balloon bursts.

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 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 ) Complete the following: 1 mol N 2 + ____ H 2 → ____ NH 3

1 mol N 2 + 3 mol H 2 → 2 mol NH 3 The balanced chemical equation tells us that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.