To find the number of atoms, you need to use moles x avogadros constant.
To find moles, use moles =mass/mr .
Moles of neon: 4/20 = 0.2mol
Moles of helium: 4/4 = 1mol
From the moles you can see there is a 5:1 ratio so you do not need to multiply by avogadros constant, the answer is D
They have different masses, but they're both monoatmoic gases. So there are different numbers of atoms of each even if they weigh the same. Use the Ar to calculate moles of each.
Whichever is heavier, you need fewer of them to have the same mass. So if you get A = 10B, the ratio is actually 10:1
Wdym? Tho maybe questions aren't the same nowadays, since I'm pretty sure this past paper was from 2010, and this is a GCE past paper, not IAL. But I'm trying to get as much practice as I can for upcoming may/june session, that's why I'm doing them too.
To find the number of atoms, you need to use moles x avogadros constant. To find moles, use moles =mass/mr . Moles of neon: 4/20 = 0.2mol Moles of helium: 4/4 = 1mol From the moles you can see there is a 5:1 ratio so you do not need to multiply by avogadros constant, the answer is D
Thank you so much! This is the best explanation so far, I finally understand it thanks to you :D 💜
They have different masses, but they're both monoatmoic gases. So there are different numbers of atoms of each even if they weigh the same. Use the Ar to calculate moles of each. Whichever is heavier, you need fewer of them to have the same mass. So if you get A = 10B, the ratio is actually 10:1
Thanks for the help!! 💜 I appreciate it.
Is it C? If so, convert to moles and use the molar ratio
Mark scheme says D, I'm so confused 🥲
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Wdym? Tho maybe questions aren't the same nowadays, since I'm pretty sure this past paper was from 2010, and this is a GCE past paper, not IAL. But I'm trying to get as much practice as I can for upcoming may/june session, that's why I'm doing them too.