Consider the following equation for the combustion of hydrogen:H₂(g) + ¹/2O₂(g) Ⓡ H₂O(g) + 243 kJIn order to produce 1215 kJ of heat, how many grams of H₂ must burn?10.0 g12.0 g0.250 g0.100 g8.00 g

Molar mass of dihydrogen= 2.01 g/ mol

Consider the following equation for the combustion of hydrogen: 2(g) + ¹/2O₂(g) ® H₂O(g) + 243 kJ n order to produce 1215 kJ of heat, how many grams of H₂ must burn? 10.0 g 12.0 g 0.250 g 0.100 g 8.00 g

Consider the following equation for the combustion of hydrogen: 2(g) + ¹/2O₂(g) ® H₂O(g) + 243 kJ n order to produce 1215 kJ of heat, how many grams of H₂ must burn? 10.0 g 12.0 g 0.250 g 0.100 g 8.00 g

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...

See similar textbooks

Related questions

Q: 1. H₂(g) + O₂(g) → 2H₂O AH = -572 kJ a. How much heat is produced in the production of 100.g of H₂O?…

A: Dear student, Since you have posted multiple questions, according to the BARTLEBY qna guidelines..…

Q: Nitric acid is neutralized with potassium hydroxide in the next reaction. HNO3(aq) + KOH(aq) →…

A: We will first determine the mass of solution by adding the volume and multiplying density. And we…

Q: Given the AH for the following reactions, P4(s) +6C12(g) →→ 4PC13 (8) AH = -2439 kJ 4PC15(g) → P4(s)…

Q: 8. The overall reaction in commercial heat packs can be represented as How much heat is released…

Q: e the information to answer the following questions. This reaction is... Suppose 41.0 g of NH3…

A: The given data: 2NH3(g) ==> N2(g) + 3H2(g)∆H° = 160 KJ When ∆H° is positive, it means heat is…

Q: Consider these reactions: Reaction 1: H2 (9) + Cl2 (g) → 2HC1(9) AH=-184.6 kJ %3D Reaction 2: 20F2…

A: ->If ∆H = +ve => reaction is endothermic reaction ->if ∆H = ,-ve => reaction is…

Q: Using the balanced equation shown below, calculate the mass of C3H8 that must react in order to…

A: According to the given reaction, the combustion of one mole of C3H8 releases 2219.9 kJ of heat. One…

Q: How much heat (in kJ) is produced by the complete combustion of 52.2 g of CH4? Use 1.01 g/mol for…

Q: How much heat is produced by the combustion of 4.67g of magnesium (24.30 g/mol)? Mg(s) + 1/2 O2(g)…

A: Here we have to apply mole concept, first we need to find for 1 gram Mg combustion how much energy…

Q: In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH), was added to 70.0 mL of 0.600 M HCl.…

A: The question is based on the concept of calorimetry . whatever heat absorbed by solution is released…

Q: How much heat is produced when 25.4 g of NO2 react? 4NO2(g) + O2(g) → 2N2O5(g) heat of…

A: Given Mass of NO2= 25.4 g To find heat is produced.

Q: How much heat is produced by the complete combustion of 264 gg of CH4CH4?

A: Given:CH4g+2O2g→CO2g+2 H2Og∆Hrxn°=-802.3 kJ

Q: Pentaborane, B5H9, was once studied as a potential rocket fuel. Calculate the heat given off when 1…

A: 2B5H9 + 12O2 ------> 5B2O3 + 9H20 Enthalpy of reaction = Sum of enthalpies of products-sum of…

Q: CS2 and 10.0 g Cl2 reacts by the followi CS2(g) + 3Cl2 (g) AH = -230. kJ

A: Given, Mass of Cl2 = 10 g Mass of CS2 = 10 g Molar mass of CS2 = 76 g/mol Molar mass of Cl2 = 71 g…

Q: Given the following reactions N2 (g) + O2 (g) → 2NO (g) 2NO(g) + O2(g) → 2N (g) the enthalpy of…

Q: Consider the following reaction: D2(g) + A2(g) → 2AD(g) AH = 237.4 kJ If 72.4 kJ of heat are…

A: The objective of the question is to find out how many grams of AD should be produced when 72.4 kJ of…

Q: The reaction 3H2(g) + N2(g) → 2NH3(g) has an enthalpy of reaction of -92.6 kJ/mol. If 2 g of…

A: According to the given balanced chemical equation, one mole of nitrogen reacts to produce 92.6 kJ of…

Q: Iron can be converted to Fe₂O₃ according to the reaction below. How much heat (in kJ) is required to…

A: The branch of chemistry that deals with the structure, properties and the reaction of the organic…

Q: Mass of water 5.678 g Ti 2.33 Tf -21.33 a. calculate the heat lost when the mass of water (g)…

A: This problem is based on phase tranfer of matter . Here water transform from water to ice from…

Q: with 2 mol O2 (g) to produce 1 mol CO2 (g), 2 mol H2O(l), and 890 kJ of heat. Write a…

A: when any substance which burns in presence of oxygen that reaction is called as combustion reaction.…

Q: Determine the amount of heat (in kJ) associated with the production of 1.76 × 104 g of NO2 according…

A: Molar mass of nitrogen dioxide is 46 g/mol

Q: How much heat is evolved when 453.5 g of ammonia (NH3) is produced according to the following…

A: Given Reaction is - N2 (g) + 3H2 (g) → 2NH3 (g) ΔH= -91.8 kJ

Q: What is the heat of a reaction, in joules, with a total reaction mixture volume of 57.5 mL if the…

A: Density of the mixture = 1 g/ml Volume of the mixture = 57.5 ml Mass of the mixture = Density of the…

Q: When carbon disulfide,CS2, forms from its elements, heat is absorbed. How much heat would be…

A: Enthalpy of formation of carbon disulphide = 89.3 kJ The formation of carbon disulphide is for 1…

Q: The combustion of CH4 releases 890.4 kJ/mol of heat according to the equation: CH4(g) + 2 O2(g) -->…

Q: For the following combustion reaction CH3CH₂CH₂COOH(1) +502(g) → 4CO₂(g) + 4H₂O(g) AH = -2.18 × 10³…

Q: Given the following: S8 (g) + O₂(g) → SO₂ (g) 3 8(g) +02 (g) → SO3 (g) The heat of reaction for SO₂…

A: To calculate the heat of reaction for given reaction, we need to modify the given two reactions for…

Q: The enthalpy change for the reaction of hydrogen gas with fluorine gas to produce hydrogen fluoride…

Q: We allow 73 g of oxygen to react with 85 g of ethane. The reaction is shown below. Since the heat…

A: Given - Balanced thermodynamical Reaction - C2H6 (g) + 7/2 O2 (g) → 2 CO2 (g) + 3 H2O (g) ,…

Q: The reaction between nitrogen and oxygen gases requires the absorption of 43 kJ of energy per mole…

A: The reactions in which heat energy is released from the system are known as exothermic reactions.…

Q: 8. The equation for the combustion of methane, CH4 (the main component in natural gas) is shown…

Q: Here is the reaction equation for the combustion of butane, which is an exothermic reaction. 2…

A: Exothermic reaction that releases energy from the system to its surroundings

Q: What is the q (heat) for 140.2 g of PCl3 decomposing to form chlorine gas and elemental phosphorus?…

A: Decomposition reaction of PCl3 is ,∆H°rxn =1207 kJMass of PCl3 = 140.2 g Molar mass of PCl3 = 137.32…

Q: Given the equation below, which of the following is true? 2 Mg(s) + O2(g) → 2 MgO(s) + 72.3 kJ 12.…

A: 2Mg + O2->2MgO+72.3KJ

Q: In the following reaction, what is the quantity of heat (in kJ) released when 1.81 moles of CH4 are…

Q: 3. When carbon disulfide, CS2, forms from its elements, heat is absorbed. How much heat would be…

A: Enthalpy of reaction - it is the heat evolved or absorbed when number of moles of reactants , as…

Q: Magnesium burns in air to produce a bright light and is often used in fireworks displays. The…

Q: Consider the following reaction: 2CH₂OH(g) 2CH4 (g) + O₂(g), AH= +252.8 kJ

A: Given -> Weight of CH3OH = 27.0 gm 2CH3OH(g) ------> 2CH4(g) + O2(g) ∆H=+252.8 KJ

Q: Charcoal is primarily carbon. Determine the mass of CO2produced by burning enough carbon to produce…

A: The given reaction is C(s) + O2(g) ------> CO2(g) ∆H = -393.5 kJ

Q: To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of…

A: Mass of sample = 704.8 mg Heat supply = 35.548 J Initial temperature = 297.05 k Final…

Q: A chemist measures the energy change AH during the following reaction: 2 NH3(g) → N₂(g) + 3H₂(g) ΔΗ=…

Q: Hydrazine, N2H4, is a liquid used as a rocket fuel. It reacts with oxygen to yield nitrogen gas and…

A: Molar mass of hydrazine (N2H4) = 32.045 g/mol

Q: What is the heat of a reaction, in joules, with a total reaction mixture volume of 69.0 mL if the…

Q: The reaction between nitrogen and oxygen gases require the absorption of 43 kJ of energy per mole of…

Q: In the following reaction, how much heat is generated when 3.27 moles of CH« are burned? CH: (g) + 2…

A: The reaction is : CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ∆H°=-802 kJ/mol Here, as we can…

Question

Consider the following equation for the combustion of hydrogen:
H₂(g) + ¹/2O₂(g) Ⓡ H₂O(g) + 243 kJ
In order to produce 1215 kJ of heat, how many grams of H₂ must burn?
10.0 g
12.0 g
0.250 g
0.100 g
8.00 g

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

For the reaction below ΔH = -296 kJ per mole of SO2 formed. S(s) + O2(g) → SO2(g) (a) Calculate the quantity of heat released when 1.75 g of sulfur is burned in oxygen.
Calculate the heat exchanged when 32.0 g oxygen reacts with 16.0 g methane: CH4(g) + 3/2 O2(g) → CO2(g) +2H2O(l) qrx= -900 kj
Consider the balanced chemical equation:2Al(s) + Fe2O3(s) -> 2Fe(s) + Al2O3(s)heat of reaction = −851.5 kJ (c) What mass of Fe2O3 must react to produce 387 kJ of heat? (d) What mass of Fe is produced at the same time 387 kJ of heat is produced?
2 Al (s) + Fe2O3 (s) → 2 Fe (l) + Al2O3 (l) ΔH = −848.0 kJ If 250. g of aluminum is consumed in the reaction, how much heat (in kJ) could theoretically be generated? Include the sign in your answer.
when butane (C4H10) in a cigarette lighter undergoes combustion, it evolves 2880 kJ per mole of butane. what is the mass of water formed if 1150 kJ of heat evolves?
In a constant-pressure calorimeter, 50.0 mL of 0.340 M Ba(OH), was added to 50.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 23.73 °C to 28.36 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H,O produced)? Assume that the total volume is the sum of the individual volumes. kJ/mol H, C 52.356 ΔΗ- Incorrect
Consider the reaction of hydrogen with sulfur to form hydrogen sulfide: 8H₂ (g) + Sg (s) → 8H₂S(g), which has an enthalpy of reaction of -20.15 kJ/mol. If 150 g of sulfur are reacted with an excess of hydrogen, how much heat is produced (kJ)?
The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) What mass of aluminum is needed to produce 664. kJ of heat ? AH = -850. kJ O 36.7 g O 31.3 g O 32.8 g O 55.3 g 42.2g • Previous Not saved MacBook Air 吕0 F1 F2 DII
In a constant-pressure calorimeter, 75.0 mL of 0.880 M H, SO, was added to 75.0 ml. of 0.440 M NaOH. The reaction caused the temperature of the solution to rise from 23.49 C to 26.49 C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/(g °C), respectively), what is AH for this reaction (per mole of H,O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,0
8CO2(g) + S13N4(s) → 8CO + 2N20 + 3SIO2 AH = +461.05 kJ a) Is this reaction exothermic or endothermic? b) What type of reaction is this? c) Is heat a reactant or product in this reaction? d) How much heat energy is produced when 5.5 g of carbon dioxide are reacted? e) What mass of N20 is produced when 3.5 g of S13N4 are reacted? f) How much heat energy is involved when 7.5 g of Si02 are produced?
Do the follow reactions depict Heat of Formation Reactions? If so, mark the reaction as YES, if it is not a Heat of Formation Reaction, then choose NO. ✓3/2 H₂(g) + P(s) → PH3(g) H₂(g) + 1/2O₂(g) → H₂O(g) Al(s) + 3/2 Br₂(1)→ AlBr3(S) Na(s) + H₂O(1)→ NaOH(aq) + 1/2 H₂(g) ✓2As(s) + 5/2 O₂(g) → As2O5(s) In formation reactions the reactants must be elements in their most common states, and the only product is one mole of the substance of interest.
Consider the following reaction: 2 H2(g) + O2(g) 2 H2O(l) Answer the following questions: (a) How much heat is evolved when 1.249×101 moles of H2O(l) is produced from the combustion of H2(g).Answer to 4 sig figs. (b) How much heat is evolved when 1.310×101 g of H2(g) is burned in excess oxygen.Answer to 4 sig figs. (c) How much heat is evolved when 1.736×102 moles of H2(g) is burned in excess oxygen.Answer to 4 sig figs.