Use the data below to calculate the total heat in kJ needed for the following processés.melting point at 1 atmspecific heat of liquid sodium 1.38 J/g°C97.80°Cspecific heat of solid sodium 1.23 J/g°CAHfus2.60 kJ/molProvide the numerical answer without units to the correct significant figures and in a 'non-exponential form, i.e., in aform 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 whenthe 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 whenthe atmospheric pressure is 1 atm.

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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How many litres of C6H14(l)C6H14(l), measured at 20 ∘C, must be burned to provide enough heat to warm 26.4 m^3of water from 18.2 to 33.1 ∘C , assuming that all the heat of combustion is transferred to the water, which has a specific heat of 4.18 J g^−1 ∘C? Recall that 1 mL=10−3 L1 mL=10−3 L. Express your answer to four significant figures and include the appropriate units.
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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.
P
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.
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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

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