The reaction: (CH3)3CBr + OH− → (CH3)3COH + Br− in a certain solvent is first order with respect to OH−. In several experiments, the rate constant k was determined at different temperatures. A plot of ln(k) vs 1/T was constructed and the slope of the line was -1.10 x 104 K with a y-intercept of 33.5. What is the activation energy for this reaction? A) -91,400 J/mol
B) -1.10 × 10⁴ J/mol
C) 1.10 × 10⁴ J/mol
D) 91,400 J/mol​

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.

Ireally don’t know this

Use the universal gas law formula: pv = nrt now, the key word in this problem is stp, so at stp, temperature will always be 0 degrees celsius and pressure will always be 1.0 atm or 760 torr. given something is at stp, we already know the two variables pressure and temperature. the other thing we can find with the given information is moles. to find moles, just divide grams by molar mass of the element. 16.0g / 2(16.00)g/mol = 0.5 moles plug the values in to the equation pv = nrt (1.0 atm)( x ) = (0.5 )(0+273=273k) the r value is just a constant for when we use atm, liters, moles and kelvin. i'm assuming you want your answer in liters, but if you dont just move the decimal 3 to the right in your final answer. so when plugging these numbers in to your calculator and trying to find x, you get 11.20665 liters using significant figures the answer is 11.2 liters