Use the data below to calculate the total heat in kJ needed for the following processés. melting point at 1 atm specific heat of liquid sodium 1.38 J/g°C 97.80°C specific heat of solid sodium 1.23 J/g°C AHfus 2.60 kJ/mol Provide the numerical answer without units to the correct significant figures and in a 'non-exponential form, i.e., in a form where the exponent is zero and therefore not shown. For example, 0.444 rather than 4.44 x 101. 1. The energy in kJ needed to heat 20.00 g of solid sodium (22.99 g/mol) at -5.00°C to solid sodium at 97.80°C when the atmospheric pressure is 1 atm. 2. The energy in kJ needed to heat 20.00g of solid sodium (22.99 g/mol) at 97.80°C to liquid sodium at 97.80°C when the atmospheric pressure is 1 atm.

2 NO(g) N2(g) + O2(g)   H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g)   H = -113.1 kJ 2 N2O(g) 2 N2(g) + O2(g)   H = -163.2 kJ Use Hess's law to calculate H for the reaction below.3 NO(g) N2O(g) + NO2(g)H = _____k J

Calculate the amount of heat needed to boil 23.1g of octane (C8H18), beginning from a temperature of 97.0°C. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol.

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In the laboratory a student finds that it takes 139 Joules to increase the temperature of 13.0 grams of solid silicon from 23.1 to 39.5 degrees Celsius.The specific heat of silicon calculated from her data is _______J/g°C.

In the laboratory a student finds that it takes 35.9 Joules to increase the temperature of 11.7 grams of solid silver from 23.8 to 37.8 degrees Celsius.The specific heat of silver calculated from her data is _______ J/g°C.

Calculate the amount of heat needed to boil 157. g of benzene (CH), beginning from a temperature of 19.0 °C. Be sure your answer has a unit symbol and the correct number of significant digits.

Please don't provide handwritten solution.....

How much heat is given off to the surroundings when 6 g of aluminum reacts according to the following equation? Express your answer correctly rounded to two decimal places.2 Al + Fe2O3  Al2O3 + 2 Fe ΔH°rxn = -849 kJ. kJIf all of the heat generated by the reaction was absorbed by one liter of room temperature water, what would be the highest temperature the water could reach? Express your answer correctly rounded to two decimal places. °CWhile writing this question, I had to take into account that the final temperature reachable in the previous question could not exceed the boiling point of water. Given this information, what is the highest whole number amount of aluminum that could have been used for this question? Enter only a number for your answer. g