[ANSWER] How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C?
Avogadro’s number = 6.022 x 1023
A. 7.01 × 1021 molecules
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[ANSWER] How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C?
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B. 7.38 × 1021 molecules
C. 2.12 × 1022 molecules
D. 2.23 × 1022 molecules
EXPERT ANSWER
“B. 7.38 × 1021 molecules.” To begin, the number of moles must be determined. The ideal gas equation will be utilized to do this. PV = nRT, where n = PV/RT. As per the question, the variables take on the following values: P = 780mmHG which is similar to 103991 Pa, V = 0.4L, T = 408.15K, R = 8314.463LPa/K.mol. When these values are substituted into the equation, the following results: n = (103991 x 0.4)/ (8314.463 x 408.15) = 0.012 moles. Since one mole possesses 6.02 × 1023 particles, 0.012 moles will comprise of 0.012 x 6.02 x 1023 molecules. This results in 7.38 × 1021 molecules.
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