Question

If the complete reaction of 45.0 g of B(s) requires 74.93 kJ of heat to be...

If the complete reaction of 45.0 g of B(s) requires 74.93 kJ of heat to be absorbed from the surroundings, what is the enthalpy change of the following equation in kJ/molrxn? 2B(s) + 3H2(g) -> B2H6 (g) ∆H rxn = ? kJ/molrxn

Homework Answers

Answer #1

2B(s) + 3H2(g) ---------------------------> B2H6 (g)

21.62 g B -----------------------> kJ

45.0 g B ---------------------------> 74.93 kJ

heat needed for the reaction = 74.93 x 21.62 / 45.0

                                               = 36.0 kJ /mol

∆H rxn = 36.0 kJ /mol

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Hess's law states that "the heat released or absorbed in a chemical process is the same...
Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." It is important to recall the following rules: When two reactions are added, their enthalpy values are added. When a reaction is reversed, the sign of its enthalpy value changes. When the coefficients of a reaction are multiplied by a factor, the enthalpy value is multiplied by that same factor. Part A Calculate...
Consider the reaction: B2H6(g) +3O2(g) ---> B2O3(s)+3H2O(g) ...........(triangle H) = -2035 KJ Calculate the amount of...
Consider the reaction: B2H6(g) +3O2(g) ---> B2O3(s)+3H2O(g) ...........(triangle H) = -2035 KJ Calculate the amount of heat released when each of the following amounts of diborane (B2H6) is burned -1.000 x 10^2 mol -1 mol
C2N2O2Hg(s) + O2 (g) -> Hg(g) + 2CO2(g) + N2(g) Determine the theoretical enthalpy (in kJ/mol)...
C2N2O2Hg(s) + O2 (g) -> Hg(g) + 2CO2(g) + N2(g) Determine the theoretical enthalpy (in kJ/mol) of the mercury fulminate reaction by using the enthalpy of formation for mercury fulminate (+ 386 kJ/mol) Remember, ΔH° rxn = Σn x H°f(products) - Σn x ΔH°f(reactants). Explain your work. We are assuming a constant pressure situation. This is can also be termed the heat of explosion, but when it is termed heat of explosion, the units are traditionally kJ/kg of substance. Convert...
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the...
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. DELTA-H =___ kJ (c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? _____g (d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g)...
30) a)how much heat is released(in kJ) when 100.0 g H2O(l) is formed from the combustion...
30) a)how much heat is released(in kJ) when 100.0 g H2O(l) is formed from the combustion of H2(g) and O2(g) 2H2(g) + 2O2(g) →2H2O(l) ∆H°=-571.6 kJ. b) in an exothermic reaction? a) heat is absorbed from the surroundings b) temperature is constant c) pressure increases d) heat is transferred to the surroundings c) which of the following does not require a heat transfer into the system? a)bond formation b) vaporization c) sublimation d) all require heat in D) doubling the...
What mass of natural gas (CH4) must you burn to emit 275 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ...
What mass of natural gas (CH4) must you burn to emit 275 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ m = Pentane (C5H12) is a component of gasoline that burns according to the following balanced equation: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g) Part A Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of liquid pentane is -146.8 kJ/mol.) Express your answer using five significant figures. ΔH∘rxn = kJ
Hess’s Law b) Calculate the ∆H for the reaction: Ti(s) + 2Cl2 (g) → TiCl4 (l)...
Hess’s Law b) Calculate the ∆H for the reaction: Ti(s) + 2Cl2 (g) → TiCl4 (l) Using the following chemical equations and their respective enthalpy changes: Ti(s) + 2Cl2 (g) → TiCl4 (g) ∆H = -763 kJ TiCl4 (l) → TiCl4 (g) ∆H = 41 kJ b) Calculate the ∆H for the reaction: 2CO(g) + O2 (g) → 2CO2 (g) Using the following chemical equations and their respective enthalpy changes: 2C(s) + O2 (g) → 2CO(g) ∆H = -221.0 kJ...
Constants | Periodic Table Learning Goal: To understand how standard enthalpy of reaction is related to...
Constants | Periodic Table Learning Goal: To understand how standard enthalpy of reaction is related to the standard heats of formation of the reactants and products. The standard enthalpy of reaction is the enthalpy change that occurs in a reaction when all the reactants and products are in their standard states. The symbol for the standard enthalpy of reaction is ΔH∘rxn, where the subscript "rxn" stands for "reaction." The standard enthalpy of a reaction is calculated from the standard heats...
Use Hess's Law to calculate the enthalpy change for the reaction: GdO3 + 3H2(g) -> Gd(s)...
Use Hess's Law to calculate the enthalpy change for the reaction: GdO3 + 3H2(g) -> Gd(s) + H2O (g) from the following data: 2Gd(s) + 3O2 --> 2GdO3(s)   ^H=-685.4kJ 2H2 (g) + O2 (g) --> 2H2O(g)     ^H= -47.8kJ
The value of ΔH° for the reaction below is -126 kJ. The amount of heat that...
The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 45.0 g of Na2O2 with water is ________ kJ. 2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT