Tetraphosphorus decaoxide, P4O10, is an acidic oxide. It reacts with water to produce phosphoric acid, H3PO4, in an exothermic reaction. P4O10(s) + 6 H2O(l) → 4 H3PO4(aq) ΔHorxn = -257.2 kJ a) Rewrite the thermochemical equation to include the enthalpy change as a term in the equation. b) How much energy is released from the reaction of 5.00 mol of P4O10 with excess water?

Tetraphosphorus decaoxide, P4O10, is an acidic oxide. It reacts with water to produce phosphoric acid, H3PO4, in an exothermic reaction. P4O10(s) + 6 H2O(l) → 4 H3PO4(aq) ΔHorxn = -257.2 kJ a) Rewrite the thermochemical equation to include the enthalpy change as a term in the equation. b) How much energy is released from the reaction of 5.00 mol of P4O10 with excess water?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 49QAP: Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make...

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Issue 1Iron(III) oxide reacts with carbon monoxide to produce elemental iron and carbon dioxide. Determine the enthalpy change for this reaction using known enthalpies of formation. Fe2O3(s) + 3 CO(g) → 3 CO2(g) + 2 Fe(s) Issue 2Tetraphosphorus decaoxide, P4O10, is an acidic oxide. It reacts with water to produce phosphoric acid, H3PO4, in an exothermic reaction. P4O10(s) + 6 H2O(l) → 4 H3PO4(aq) ΔHorxn = -257.2 kJ a) Rewrite the thermochemical equation to include the enthalpy change as a term in the equation. b) How much energy is released from the reaction of 5.00 mol of P4O10 with excess water? Issue 4Find, using Hess's law, the overall enthalpy change of the reaction below. Determine whether the reaction is endothermic or exothermic. 2N2 + 5O2 → 2N2O5 Refer to the following reactions. 1) 2H2O → O2 + 2H2 ∆H= +572 kJ 2) N2O5 + H2O → 2HNO3 ∆H= -78 kJ 3) N2 + 3O2 + H2 → 2HNO3 ∆H= -349 kJ Issue 5The data in the table below was compiled for the following reaction. A + B → C + D…
Select all that is true for thermochemical equations. A. If the coefficients in a balanced equation are multiplied by 2, the enthalpy change must also be multiplied by 2. B. If a reaction is endothermic and the equation for the reaction is reversed, the enthalpy change becomes positive. C. If there is 1 mole H2O(l) on the reactant side of the equation and there is 1 mole H2O(g) on the product side, they are canceled from the equation. D. There are two ways to express thermochemical equations--one with the heat on the reactant or product side of the equation and one with delta H equals the heat change.
1. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? answer: -550. cal (or -2.30 x 103 J) 2. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? answer: 3.00 x 103 cal (or 1.26 x 104 J)
Consider the following reaction: 2 CH3OH(g) → 2 CH4(g) + O2(g) DH = 252.8 kJ (a) Is reaction exothermic or endothermic? ANSWERED (b) Calculate the amount of heat transferred when 24.0 g of CH3OH(g) is decomposed by this reaction at constant pressure. ANSWERED (c) For a given sample of CH3OH, the enthalpy change during the reaction is 82.1 kJ. How many grams of methane gas are produced? ANSWERED (d) How many kilojoules of heat are released when 38.5 g of CH4(g) reacts completely with O2(g) at constant pressure?
How much energy is required to raise the temperature of 10.9 grams of solid zinc from 22.5 °C to 35.7 °C ?Answer: Joules.
A calorimeter was filled with 50 g of water with an initial temperature of 10 °C then hot water weighing 100 g and a temperature of 99 °C was introduced. The system was allowed to reach equilibrium and the final temperature was 68 °C. What is the specific heat of the calorimeter in J/g °C? Report answer with three significant figures.
Can you help me? 4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? Answer: -550. cal (or -2.30 x 103 J) 5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? Answer: 3.00 x 103 cal (or 1.26 x 104 J) 6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 cal
If 25.6 J of energy raised 786 g of a substance from 20.0o C to 35.0o C, what is the specific heat of the substance (S)? Answer: 2.17 x 10-3 J/g °C
4. How much energy is removed from 500.0 g of water when the temperature is lowered by 1.10 o C? Answer: -550. cal (or -2.30 x 103 J) 5. How much energy is required to raise the temperature of 1000.0 g of water from 23.00 o C to 26.00 o C? Answer: 3.00 x 103 cal (or 1.26 x 104 J) 6. The specific heat of copper is (0.0924 cal/go C), how much energy is required to raise the temperature of 10.0 g of copper by 100.0 o C? Answer: 92.4 cal
If ethanol (15.0 g) is burned, how much heat is released? Ethanol MW = 46.07 g/mol C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH°rxn = –1367 kJ/mol Answer: 445 kJ, just need steps TY!
2 A 30.5 gram sample of an alloy at 93.0 C is placed into 50.0 grams of water at 22.0 C in an insulated coffee-cup calorimeter with a heat capacity of 9.2 J/C. If the final temperature of the system is 31.1 C, what is the specific heat of the alloy? ( CH2O = 4.184 J/g-C). (Enter the number only keep sig fig)
What is the specific heat capacity of a substance of mass 176.1 g that increases in temperature from 20.8 °C to 27.7 °C after absorbing 2.76 kJ of energy in the form of heat? Express your answer in J g-1 °C-1. Do not try to identify the substance. Express answer in 2 significant figures.