Assuming the combustion of hydrogen gas provides three times as much energy pergram as gasoline, calculate the volume of liquid H2 (density = 0.0710 g/mL) requiredto furnish the energy contained in 120.0 L of gasoline (density = 0.740 g/mL)O 277 L320 LO 417 LO None of the above120 L Question 3 (2 points)The pressure of a gas is measured as 89 torr. Represent this pressure in bothatmospheres and pascalsO 1.17 x10^-1 atm; 1.19 x10^4 PaO 1.19x 10^ 4 atm; 1.17 x 10^-1 Pa6.4 x 10^-2 atm, 6.5 x 10^3 paNone of theseO 1.49x 10^ 4 atm; 2.67 x 10^-1 Pa

Hello. Since your question has multiple questions, we will solve the first question for you. If you…

Assuming the combustion of hydrogen gas provides three times as much energy per gram as gasoline, calculate the volume of liquid H2 (density = 0.0710 g/mL) required to furnish the energy contained in 120.0 L of gasoline (density = 0.740 g/mL) O 277 L 320 L | 417 L O None of the above 120 L

Assuming the combustion of hydrogen gas provides three times as much energy per gram as gasoline, calculate the volume of liquid H2 (density = 0.0710 g/mL) required to furnish the energy contained in 120.0 L of gasoline (density = 0.740 g/mL) O 277 L 320 L | 417 L O None of the above 120 L

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

Similar questions

The burning of 1.5 g of vegetable cause the temperature of 58.18 g of water in a soda can calorimeter to increase from 21.5 C to 28.1 C. Calculate the amount of heat absorbed by the water using the specific heat of water at 4.18 J/g C.
A gas expands and does work on the surroundings equal to 3.55 L atm. At the same time, it releases 540.4 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
A 6.61g sample of an unknown salt (MM=116.82g//mol) is dissolved in 150.00g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 C. After the salt has completely dissolved, the temperature of the solution is 28.54 C. Given that 156.61 g of solution increased in temperature by 4.82 °C, what quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g• °C.
Enter your answer in the provided box. A gas expands and does P-V work on the surroundings equal to 299 J. At the same time, it absorbs 196 J of heat from the surroundings. What is the change in energy of the system? J
Classify the reaction endothermic or exothermic and give the change in enthalpy of the reaction. CH3OH (1) + 3 O₂ (g) → 2 CO₂ (g) + 4 H₂O (g) Δ Η = -557 kJ The heat energy in the reaction is Select an answer This makes the reaction Select an answer So, the energy would be on the Select an answer side.
A student is asked to identify an unknown piece of metal. The metal has a mass of 12.34 g. It is placed in a boiling water bath and brought up to 99.98 oC. A coffee-cup calorimeter is set up with 103.25 mL of water (density = 1.00 g/mL and specific heat = 4.184 J/g.oC) at a room temperature of 21.30 oC. The metal is removed from the boiling water and placed in the calorimeter. A final temperature is recorded as 22.32 oC. Find the specific heatcapacity of the unknown metal. (Assume there is no heat loss)
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
A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.73 kj/°c. When a 0.26-g sample is used, the temperature change is 10.5°C. What is the energy density of the sample in k/g? Round your answer to 2 decimal places.
Classify the substances below as reactants or products and state their state of 2NaHCO3 (s) → Na,CO3 (s) + H20 (1) + CO2 (g) matter:
1. A thermometer placed in a solution undergoing a chemical reaction indicates an increase in temperature as the reaction proceeds. Is this reaction endothermic or exothermic? Describe if heat energy is lost or gained from the reaction (the system) to the surroundings. What is the sign of the enthalpy change (AH) of this reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand will become cold. a) Is the reaction H,O(s) – H,O(1) endothermic or exothermic? b) In which direction does heat flow?
Determine the most likely identity of the unknown metal sample. Mass of empty beaker = 50.45 g Mass of beaker and water = 81.26 g Mass of water 30.81 g (represents a calculation rather than a direct measurement) Initial water temperature = 25.5 C Mass of metal = 54.02 g Initial metal temperature = 102.5 C Final water and metal mixture temperature = 36.0 C The specific heat capacity of water is 4184 J/kg C