Here, Molar mass of N2O4 = 92.02 g/mol
So, Number of molecules in 1 mole (92.02 g) = 6.023 * 10²³
Number of molecules in 76.3 g = 6.023 * 10²³ / 92.02 * 76.3
= 6.023 * 10²³ / 1.20
= 5 * 10²³
In short, Your Answer would be approx. 5 * 10²³ molecules
Hope this helps!
Answer:
The new volume is 7.27 L
Explanation:
Step 1: Data given
The initial volume of the balloon = 7.0 L
The pressure = 765 mmHg = 765/760 atm = 1.00658 atm
The pressure drops to 737 mmHg = 737/ 760 atm = 0.969737
The temperature remains constant
Step 2: Calculate the new volume
P1*V1 = P2*V2
⇒with P1 = the initial pressure in the balloon = 765 mmHg
⇒with V1 = the initial volume = 7.0L
⇒with P2 = the decreased pressure = 737 mmHg
⇒with V2 = the new volume = TO BE DETERMINED
765 mmHg * 7.0 L = 737 mmHG * V2
V2 = (765 mmHG * 7.0 L) / 737 mmHG
V2 = 7.27 L
The new volume is 7.27 L
Element. Everything is else is a mixture, therefore not pure.
Answer:
Answer is option C
Explanation:
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D is the correct answer
every other option contains an element
