(1) 1.0g magnesium reacts with water to release heat of14.7kj. The faster the reaction speed, the greater the heat released and the higher the solution temperature. Because only the specifications of magnesium are different in curves 1, 2 and 3, the factors affecting the reaction rate of magnesium with water are: the reaction surface area of magnesium,

So the answer is: d;

(2) According to the image in Figure 3, after adding 0. 125mol sodium chloride, the temperature of the solution has reached the boiling point, so the experiment with the dosage greater than 0.125mol sodium chloride will not be done.

So, the answer is: c;

(3) As can be seen from Figure 3, when 0.060mol NaCl is added, the reaction temperature is more than 40℃ and less than 50℃, and the temperature of the mixture is closest to 42℃.

So, the answer is: b;

(4) Magnesium powder heats up faster than magnesium bars. When magnesium and sodium chloride are fixed, the reaction temperature reaches the maximum when 0.50mol iron powder is added to 0. 1mol magnesium, and excessive iron powder will cause waste, so A is correct.

So, the answer is: a;

(5) 1.0g magnesium reacts with water to give off heat of 14.7kJ, and 24g magnesium gives off heat of 352.7kJ The thermochemical equation of flameless heater reaction is: mg (s)+2h2o (l) = mg (oh) 2 (s)+H2 (g) △ h =-.

The answer is: mg (s)+2h2o (l) = mg (oh) 2 (s)+H2 (g) △ h =-352.8kj/mol;

(6) Magnesium, iron powder and NaCl solution constitute a primary battery, which can greatly speed up the reaction, so the answer is that magnesium, iron powder and NaCl may constitute a primary battery.