Enter your answer in the provided box. the vapor pressure of ethanol is 1.00 x 10² mmhg at 34.90°c. what is its vapor pressure at 54.81°c? ( ah yap for ethanol is 39.3 kj/mol.) mmhg

2,54x10² mmHg

Explanation:

To solve this problem you can use Clausius-Clapeyron equation that serves to estimate vapor pressures or temperatures:

Where:

P1 is 1,00x10² mmHg

ΔHvap is 39,3 kJ/mol

R is gas constant 8,314x10⁻³ kJmol⁻¹K⁻¹

T1 is 34,90°C + 273,15 = 308,05 K

T2 is 54,81°C + 273,15 = 327,96 K

Thus:

Thus, P2 is 2,54x10² mmHg

I hope it helps!

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.