Given for this problem: Element R has a molecular weight of 72.00   Note!! Element R is not a real element. Element A has a molecular weight of 22.00   Note!! Element A is not a real element. Given the reaction  2R + 3A  =   R2A3 q = mass X specific heat X (Tfinal - Tinitial)

If 0.24 mols of substance B is able to produce 137J of heat. What is the change in reaction enthalpy in J associated with the following balanced reaction. (Hint: *pay attention the the coefficient for substances B *determine the sign for heat, is it + or -). Round and report your answer to an integer without decimal place including + or- - sign. Only enter numeric value, no unit. A+2B → AB2 + heat AHren =???

I need hand written solution only

Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining

The heat gained by the solution in  reaction two is 5.3 kJ. how many moles of NaOH were consumed ? what was the enthalpy of reaction ? (In kJ/mole)

22. Statement A: The system loses 726 J to the surroundings as heat. The enthalpy change for the system is positive. Statement B: The system absorbs 178 J to the surroundings as heat. According to sign conventions heat is negative.   Which of the following conclusions is correct about statements A and B?   Group of answer choices Statement A is incorrect, Statement B is correct. Both statements are correct. Both statements are incorrect. Statement A is correct, Statement B is incorrect.

Answer correctly in 15 mint plz

When 3.8 g A are reacted with 8.5 g D,  according to the balanced chemical equation below, 33 kJ of energy are released.  Please calculate the enthalpy for this reaction when 3 moles of G are produced.  2A + 3D = 2Z + 3G  given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole

AH° = -1670 kJ/mol 2. For this unbalanced chemical reaction: X(s) + 3/2 Y2(g) → X₂Y3 (S) 1. Calculate the mass in kg unit of X(s) that reacted with excess amount of Y₂ when 5650 kJ of heat is evolved. (A.W. for X and Y is equal 27 and 16 g/mol, respectively? 2. Explain, if the reaction is endothermic or not?

33) Coksider a neutral atom with 30 protons and 34 neutrons. The atomic number of the element is protom 53) A) 30 B) 32 C) 34 D) 64 E) 94 54) When 100.0 g of gasoline undergoes combustion, 9560 kJ of energy are released. Express the heat released in kilocalories. (Given: 4.184 J = 1 cal) 54) B A) 4.00 x 107 kcal B) 2.28 x 103 kcal C) 2.28 x 106 kcal D) 2.28 x 109 kcal E) 4.00 x 104 kcal