Because the primary product of burning hydrogen is water, hydrogen is desirable as a clean-burning fuel. Most hydrogen in the United States is produced by a process called steam-methane reformation. The reaction takes place at high temperatures (700-1000 °C). The overall reaction of steam-methane reformation is: CH4 + 2 H2O → CO2 + 4 H2 This reaction absorbs energy. Combined with the energy to heat the water, it takes about 94 kJ/mol to form hydrogen gas using steam-methane reformation. Suppose a combustion engine gets 72 kJ of work out of every mole of hydrogen gas it burns. Comparing this to the amount of energy that went into making the hydrogen, what is the efficiency of the entire process of forming, burning, and using the energy from the hydrogen? Round your answer to the nearest percent.