Consider the following system, which is at equilibrium, 3C(s) + 3H2(g) ↔ CH4(g) + C2H2(g) The result of removing some CH4(g) and C2H2(g) from the system is that

Which of the following statements about the equilibrium constant is incorrect?

Calculate the ?G°rxn using the following information.2 H2S(g) + 3 O2(g) ? 2 SO2(g) + 2 H2O(g)?G°rxn = ? ?G°f (kJ/mol)-33.4 -3300.1-228.6

If the products have a higher energy than the reactants ___________.

A reaction has an activation energy of 40 kJ/mol. What happens to the rate if you increase the temperature from 70 °C to 90 °C?

The reaction mechanism proposed for the decomposition of H2O2 is H2O2 + I- → H2O + IO- (slow) H2O2 + IO- → H2O + O2 + I- (fast) Which statement is true?

Consider the following reaction at constant P. Use the information here to determine the value ofSsurr at 398 K. Predict whether or not this reaction will be spontaneous at this temperature. 4 NH3(g) + 3 O2(g) ? 2 N2(g) + 6 H2O(g)H = -1267 kJ

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:2NO2 ? 2NO + O2In a particular experiment at 300 °C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate ofdisappearance of NO2 for this period is __________ M/s.

What is the pH of a buffer solution prepared by taking 0.292 M of acetic acid (pKa = 4.76) and 0.179 M of sodium acetate.

Nitrogen monoxide reacts with bromine at elevated temperatures according to the equation 2NO(g) + Br2(g) → 2NOBr(g) In a certain reaction mixture, the rate of formation of NOBr(g) was found to be 4.50 × 10-4 mol L-1 s-1. What is the rate of consumption of Br2(g)?